General Chemistry Organic

Please mark the correct answer

• 5.75M
• Acetate
• Acetic acid
• 1.00M
• All of the above
• None of the above

How many atoms are in 3.50 moles of Ni?

• Cannot be determined
• 205.41
• 6.02*1023
• 21.07*1023

Group IA elements have the lowest ionization energies.

• True
• False

The main difference between the condensed states and the gaseous state of matter is the distance between molecules.

• True
• False

_____________ measures the randomness within a system.

• Enthalpy
• Heat
• Gibbs Free Energy
• Entropy

True or False: Beta emission results in the formation of an element with 1 additional neutron

• True
• False

The following model explains how the temperature affects the rate constants of a chemical reaction:

• Brownian Model
• Rutherford's Atomic Model
• Crystalline Model
• Collision Model

If 2 moles of AB4were made to react with 2 moles of C2, 1 moles of AC2 will be produced.

• True
• False

When a car rolls down from a hill, ___________________ increases?

• Work
• Potential energy
• Heat
• Kinetic energy

According to the quantum theory, energy is always expressed in integral multiples.

• True
• False

Atomic number plus the number of neutrons is referred to as:

• Atomic number
• None of the choices
• Isotopes
• Mass number

Effective nuclear charge is the nuclear charge felt by an electron when both the actual nuclear charge and the repulsive effects of the other electrons are taken into account.

• True
• False

We cannot write Lewis symbols for what group of elements?

• Transition metals
• Lanthanides
• Actinides
• All of the choices

Which of the following statement is true regarding atoms?

• All of the above
• Every atom does not have net electrical charge, thus the number of electrons and protons are equal in number.
• Nucleus contains majority of the mass of an atom
• Both protons and neutrons reside inside the atom's nucleus

What is the subshell notation for quantum numbers n=3 and l=2?

• 3d
• 3f
• 4f
• 4d

It is a type of system that can transfer both mass and energy with its surroundings

• Open System

Which of the following is not an exception to the octet rule?

• Molecules with odd number of electrons
• Molecules with eight electrons in its valence shell
• Molecules with less than an octet number of electrons
• Molecules with more than an octet number of electrons

Why do some covalently bonded molecules turn out to be bipolar?

• Electrons would spend more time in one atom than the other. This creates the polarity.
• Electrons tend to form bonds and stick together in one place
• Electrons cause attraction with protons, causing them to have increased influence in the molecule
• None of the choices

We can write Lewis symbols for what group of elements?

• None of the above
• Lanthanides
• Transition metals
• Actinides

He was a German physicist and a mathematician and one of the crucial founder of thermodynamics stated that heat by itself cannot pass from a colder to a hotter body

• Rudolf Julius Emmanuel Clausius
• Lord Kelvin
• Nicolas Leonard SadiCarno
• Julius Robert von Mayer

Consider the reaction below

• Ksp = [NH4+(aq)][SO42-(aq)]
• Ksp = [NH4+(aq)]2[SO42-(aq)]
• Ksp = [NH4+(aq)][SO42-(aq)]2
• Ksp = [NH4+(aq)]2[SO42-(aq)]2

Which of the following describes the energy and 3-dimensional regions around the nucleus where an electron can be found?

• Atomic numbers
• Mass numbers
• Quantum numbers

For the given reaction mechanism, NO3 is one of the final products.

• True
• False

Which of the following quantum numbers describes the orientation of the orbitals?

• Principal quantum number
• Angular momentum quantum number
• Magnetic quantum number

Due to little space in between molecules, solids and liquids lack shapes and volume.

• True
• False

What factor affects the polarizability of a certain nonpolar molecule?

• The number of electrons in the cloud
• How dispersed are the electrons surrounding the molecule
• The molar mass of the molecule
• All of the choices

Explain the relationship between the number of bonds and the distance between bonded molecules.

• The higher the number of bonds in a molecule, the shorter the distance of molecules.
• All of the above
• The number of bonds in a molecule has no impact on the distance of molecules.
• The higher the number of bonds in a molecule, the farther the distance of molecules.

Transitioning of a particular substance from liquid phase to its gaseous phase is called?

• Evaporation
• Freezing
• Solidification
• Condensation

What are the types of systems

• Open System
• All of the choices
• Isolated System
• Closed System

Which of the following best describes the Le Chatelier's Principle?

• A body in motion will remain in motion unless an outside force acts on it.
• A body at rest will remain at rest unless an outside force acts on it.
• Chemical reactions occur when molecules collide with sufficient kinetic energy.
• If stress is imposed on a system at equilibrium, the equilibrium position of the reaction shifts to a direction that tends to lessen the stress.

It is the sum of potential and kinetic energy in a system.

• Internal energy
• Enthalpy
• Free Energy Change
• Gibbs Free Energy

Which of the following statement is true regarding Ideal Gas Law?

• All of the above
• Proportionality constant is referred to as the gas constant and is denoted by the letter R.
• None of the above
• It is a combination of Boyle's, Charle's and Avogadro's Law

Which of the following is true about d orbitals?

• No correct answer
• All d orbitals have 2 different shapes.
• Both of the given statements are correct
• All d orbitals are spherical in shape.

Amphoteric property is defined as the ability of a compound to function as a base or as an acid, depending on the solution.

• True
• False

The percent composition by mass of ferrous sulfide, FeS, is 50% Fe and 50% S.

• True
• False

Which of the following statement is true regarding Boh's Theory of the Hydrogen Atom?

• The farther away the electron is from the nucleus, the higher the excited state is.
• All of the above
• The electron is only allowed to occupy orbits of specific energies.
• Principal quantum number is expressed in integers

It is the sum of internal energy and the product of pressure and the change in volume of the system under constant pressure

• Enthalpy

Pressure is defined as the effect of a force applied to a surface and can be measured by means of a barometer or manometer.

• True
• False

Le Chatelier's principle states that if stress (or a change in condition) is imposed on a system at equilibrium, the equilibrium position shifts to a direction that tends to lessen the stress.

• True
• False

What happens during a chemical equilibrium?

• Concentration of products and reactants are at their lowest possible value.
• Concentration of products and reactants no longer have apparent change.
• Concentration of products and reactants are at their highest possible value.
• Concentration of products, reactants, and catalyst are at their highest possible value.

What is the rate law of the second step?

• k2[NO2Cl][Cl2]
• k2[NO2Cl][Cl]
• k2[NO2][Cl2]
• k2[NO2Cl]

Gases take up volume and shape of its container, are considered the least compressible state of matter and have the lowest density compared to solids and liquids.

• True
• False

Molar heat capacity is the amount of heat needed to raise the temperature of 1 mole of a substance by 1K or one degree celsius.

• True
• False

The stronger the intermolecular forces, the higher the surface tension.

• True
• False

Calculate the pH at the equivalence point when 15.0 ml of 0.200 M HCl is titrated with 0.200 M NH3.

• 5.1
• 3.2
• 2
• 6.7
• 4.3

It is the specific part of the universe that is involved in the chemical process.

• System

What traits can be observed with gases, due to the large amount of space in between molecules and the lack of interaction between them?

• Gases have low density
• Gases are expandable
• All of the above
• Gases are easily compressible

This concept was developed after a French Chemist, Claude Louis Berthollet (1803) found that some chemical reactions are reversible.

• Chemical Equilibrium

What theory explains that when certain metals are exposed to light of at least a certain minimum frequency, electrons are ejected from its surface.

• Bohr's theory of the hydrogen atom
• Heisenberg Uncertainty Principle
• Photoelectric Effect
• Aufbau Principle

What is the difference between homogeneous and heterogeneous catalysis?

• A heterogeneous catalysis occurs when gaseous reactants are adsorbed on the surface of a solid catalyst while a homogeneous catalysis occurs when reactants and catalyst have the same phase.
• None of the above
• A heterogeneous catalysis occurs when reactants and catalyst have the same phases while a homogeneous catalysis occurs when reactants and catalyst have the different phase.

In order for a given exothermic chemical reaction to proceed, heat must be supplied for the molecules to collide.

• True
• False

This refers to the capacity of an atom to attract electrons to itself.

• Electronegativity
• None of the above
• Electromagnetism
• Bond polarity

It is the study of the energy and heat associated with chemical reactions and physical transformations.

• Thermochemistry

Which of the following group of elements are Lewis structures not applicable?

• All of the choices
• Lanthanides
• Actinides
• Transition metals

Which of the following statement is true?

• All of the above
• Ionic radius is referred to as the radius of a cation or an anion
• Atomic radius is referred to as one-half the distance between the two nuclei in two adjacent metal atoms or in a diatomic molecule
• None of the above

True or False: The number of neutrons determines the identity of the element.

• True
• False

Which of the following describes the relation between reactant concentration and time in the following equation?

• PCl3 and Cl2 increase over time.
• PCl5 increase over time.
• PCl3 and Cl2 decrease over time.
• PCl5 decrease over time.

Compute for the work done if the change in internal energy is equals to 500J while giving off 350J of heat.

• 150J
• -850J
• 850J
• -150J

As long as we use stoichiometric amounts of reactants in a reaction carried out in the laboratory, we are guaranteed to get the theoretical yield of the reaction.

• True
• False

Defined as the thermodynamic potential that can be used to calculate the maximum of reversible work that may be performed by a thermodynamic system at a constant temperature and pressure

• Gibb’s Free Energy

Iron, Fe, has an atomic mass of 55.85 amu therefore, the molar mass of Fe is 55.85 g/mol.

• True
• False

A 0.10 M Benzoic acid is prepared in water at 25°C. Calculate the concentration of the acid and conjugate base, benzoate, in the solution at equilibrium. (Ka = 6.3×10-5)

• benzoic acid = 0.089; benzoate = 0.02M
• benzoic acid = 0.098 M; benzoate = 0.002 M
• benzoic acid = 0.010M; benzoate = 0.003M
• benzoic acid = 0.008M; benzoate = 0.001M

It is also called as the Nernst's Theorem.

• Spontaneous Processes
• The Second Law of Thermodynamics
• The Third Law of Thermodynamics
• Enthalpy

Concentration of reactants is reduced over the course of reaction.

• True
• False

The f-subshells of transition metals are incompletely filled.

• True
• False

Choose the pair that will serve as the cathode

• Pb/PbCl2
• Cu/CuCl

Ammonia, NH3, is a clear, colorless gas with a pungent smell produced by the reaction of hydrogen gas, H2 and nitrogen gas, N2. Which of the following chemical equation best represent this reaction?

• H2(g) + N2(g) → NH3(g)
• 3H2(g) + 3N2(g) → 2NH3(g)
• H2(g) + N2(g) → N2H2(g)
• 3H2(g) + N2(g) → 2NH3(g)

Compute the area given the following measurements: 2.0546 cm and 4.3 cm. Express the answer in significant figures.

• 8.83 cm2
• 8.8 cm2
• 8.8348 cm2
• 8.9 cm2

The electron configuration influences the properties of the elements.

• True
• False

As the mass or speed increases, kinetic energy decreases.

• True
• False

Which of the following has the highest atomic radii?

• As
• K
• Ca
• Kr

One mole of N2 contains 2*6.022 x 1023 molecules.

• True
• False

What is the mass number of an atom that has 2 protons, 2 electrons and 4 neutrons?

• 4
• 6
• 8
• None of the choices

Equivalence point is the point in acid-base titration where the concentration of the acid is equal to the concentration of the base.

• True
• False

Which of the following statement is correct?

• No correct answer
• Molecular formula shows only the relative ratio of each of each atom in a molecule
• Both of the given choices are correct
• Empirical formula shows the actual number of atoms in a molecule.

It is the sum of the potential and kinetic energy in the system.

• Internal Energy

Determine each nuclear transmutation

• K-Capture
• Positron Emission
• Alpha emission
• Beta emission

Differential Rate Law expresses how the reaction rate depends on the concentration while the Integrated Rate Law expresses how the concentrations depend on time.

• True
• False

Ideal Gas Law is expressed as PV=nRT.

• True
• False

It is the state function that measures the “hotness” or “coldness” of a substance

• Temperature

Which of the following is the correct formula of sulfurous acid?

• HSO3
• HS
• H2SO3
• H2S

During a chemical equilibrium, concentrations of products and reactants no longer have apparent change.

• True
• False

Partial pressure is defined as the amount of pressure exerted by each component gas in a mixture, which is independent of the pressure exerted by the other gases.

• True
• False

The direction of the reaction favored when stress is applied is towards the direction where the stress is lessened.

• True
• False

Please mark the correct answer If the Ka of acetic acid is 1.8x10-5 and the pH of the buffer is 5.50, what are the concentrations of acetic acid and acetate?

• Acetic acid
• Acetate
• 1.00M
• 5.75M
• All of the choices
• None of the choices

It is defined as the values of all relevant microscopic properties.

• Entropy

Which of the following is an exception to the octet rule?

• All of the above
• Molecules with odd number of electrons
• Molecules with less than an octet number of electrons
• Molecules with more than an octet number of electrons

At 25°C, in an acidic condition, Kw will always be less than 1.0×10-14.

• True
• False

How many moles of Al is needed to produce 4 moles of Al2O3

• 1 mole
• 8 moles
• 4 moles
• 2 moles

What is the relationship between polarizability and intermolecular forces?

• The higher the polarizability of a certain molecule, the stronger the intermolecular force it creates.
• The higher the polarizability of a certain molecule, the weaker the intermolecular force it creates.
• The lower the polarizability of a certain molecule, the stronger the intermolecular force it creates.
• None of the above

What is the relationship between intermolecular forces and surface tension?

• Weaker intermolecular forces result in higher surface tension
• Stronger intermolecular forces result in higher surface tension
• Stronger intermolecular forces result in lower surface tension
• Intermolecular forces have no impact on surface tension

Which of the following are characteristics of gases?

• Most compressible state of matter
• When kept in a single container, gases will mix uniformly and totally
• All of the above
• Take up volume and shape of its container

Which of the following is TRUE?

• Solutions already have more disordered molecules as compared to its pure solvent counterparts.
• Having higher solute concentrations causes lower vapor pressures.
• Solutions need a higher boiling point to evaporate as compared to their pure solvent counterparts
• All of the choices

Which ion is not correctly named?

• Fe3+, iron (III) ion
• O22-, peroxide ion
• Ca2+, calcium (II) ion
• Cr3+, chromium (III) ion

What is the mass number of an atom that has 5 protons, 5 electrons and 6 neutrons?

• None of the choices
• 10
• 16
• 11

______________ are elements located in rows, while ________ are elements located in columns

• gases; period
• no correct answer
• group; period
• period; group

True or False: Electron capture decay results in the decrease in the atomic number.

• True
• False

What is a supersaturated solution?

• A solution containing solute more than the maximum capacity a solvent can dissolve
• None of the above
• A solution containing solute lower than the maximum capacity a solvent can dissolve
• A solution having the maximum amount of solute a solvent can dissolve

Explain the relationship with bond enthalpy and the number of bonds.

• The number of bonds in a molecule has no effect on bond dissociation energy
• None of the above
• The higher the number of bonds in a molecule, the lower the needed bond dissociation energy to break them.
• The higher the number of bonds in a molecule, the higher the needed bond dissociation energy to break them.

AB4+2C2->AC2+2B2C. If 100 grams of AB4 reacts with excess of C2, it will produce 100 grams of AC2.

• True
• False

True or False: Uranium-235 and Plutonium-235 are isotopes

• True
• False

Using the periodic table, which element is in Group 4A period 6?

• Ti
• Pb
• Sn
• V

Which of the following is a characteristic of a buffer?

• 1 and 2
• 2 and 4
• 3 and 4
• 1 and 3

Elements are arranged in the periodic table in order of increasing atomic number.

• True
• False

Naproxen sodium, C14H13NaO3, is an anti-inflammatory drug used to relieve pain and swelling. It has a molar mass of 252.245 g/mol. It is usually sold in tablet form, containing 550.00 mg of the active. How many moles of naproxen sodium are in a tablet?

• 2.18x10-3moles
• 0.92x10-3 moles
• 0.46x10-3 moles
• 4.36x10-3 moles

How many significant figures are in 0.000187?

• 4
• 6
• 5
• 3

It is the type of system that can transfer energy but not mass to its surroundings.

• Closed system

What are the forces observed in capillary action:

• Adhesion
• Cohesion
• All of the above
• None of the above

This type of bond happens when an electron from an atom transfers to another atom, forming ions and creating electrostatic attraction:

• All of the choices are correct
• Covalent bond
• None of the choices
• Ionic bond

What is the collective term for forces that attracts molecules together?

• Dipole interaction
• Intermolecular forces
• Dispersion forces
• Intramolecular forces

In the following reaction, which happens first? 2NO(g) → N2O2(g)

• N2O2(g) + O2(g) → 2NO2(g)
• 2NO(g) + O2(g) → NO2(g)
• 2NO(g) +O2(g) → 2NO2(g)
• 2N2O2(g) + O2(g) → 2NO2(g)

Positive ΔH means that heat is lost from the system into its surroundings, while negative enthalpy ΔH means that heat is absorbed by the system from its surroundings

• True
• False

Which state of matter has a definite volume and shape?

• None of the above
• Gas
• Solids
• Liquids

Supersaturated solutions contain more than the maximum amount of solvent in a solution.

• True
• False

Which of the following statement is true regarding matter?

• Intensive property depends on the amount of matter being observed.
• Solutions are also referred to as homogenous mixture.
• Flammability is an example of physical property.
• Temperature is an example of extensive property.

_____________ refers to a measure of how closely individual measurements are to the actual or true value, while _______________ refers as to how closely individual measurements are to each other.

• Accuracy; precision
• Precision; accuracy

The differential rate law expresses how the reaction depends on concentration while integrated rate law expresses how concentration depends on temperature.

• True
• False

Aluminum oxide, Al2O3, is synthesized by the reaction of aluminum, Al, and oxygen gas, O2. Which of the following equations correctly represent the reaction?

• 2Al + 3O2 → 2Al2O3
• 4Al + 3O2 → 2Al2O3
• Al + O2 → Al2O3
• 2Al + O3 → Al2O3

Changes in concentration, temperature, pressure, and time are important factors to consider in chemical equilibrium.

• True
• False

This refers toa process where molecules of a solvent pass through a semipermeable membrane:

• Osmosis
• Osmotic pressure
• None of the above
• Effervescence

It is the quantity of space being occupied by matter.

• Temperature
• Energy
• Pressure
• Volume

Determine if the transformation is an Oxidation, Reduction or Neither :

• Neither
• Reduction
• Oxidation

Collision Model explains which of the following conditions:

• It explains how the catalyst affects the rate constants of a chemical reaction.
• It explains how the intermediate affects the rate constants of a chemical reaction
• It explains how the temperature affects the rate constants of a chemical reaction
• None of the above

It is the process capable of proceeding in a given direction without the help of outside energy

• Spontaneous Process

Which of the following statement is not true according to Dalton's atomic theory ?

• None of the choices
• Elements are made up of extremely tiny particles called atoms.
• Atoms are can be created or destroyed in a chemical reaction.
• Compounds are made up of a combination of atoms of more than one element
• All atoms of a given element are the same, but atoms of one element are different from the atoms of all other elements.

Compute for the area of the a rectangle, with the correct answer in significant figures.

• 22.691m2
• 23m2
• 22.69m2
• 22.6912m2

Which of the following is true for ionic bond formation?

• It is exothermic
• It doesn't need energy to form
• It is endothermic
• None of the above

When ΔS > 0 and ΔH < 0, the process is _________________________.

• Hard to tell
• Non-spontaneous
• None of the choices
• Spontaneous

Using the periodic table, which element is in Group 2A period 5?

• Sr
• N
• Ba
• Ra

True or False: Alpha emissions result in the release of gamma rays.

• True
• False

The magnetic quantum number describes the size of the orbital. It also indirectly describes the energy of an orbital.

• True
• False

Compute the change of internal energy of a certain process in which 3000 J of heat is added to a system while the system does work equivalent to 6000 J by expanding against the surrounding atmosphere.

• -3000J
• 9000J
• 3000J
• -9000J

Given the percent composition by mass of all the elements in an unknown compound, we can always determine its molecular formula.

• True
• False

It is the properties that are determined by the state of a system regardless of how that condition was achieved.

• Spontaneous Process

A melting ice is an example of the first law of thermodynamics.

• True
• False

Which of the following statements is false?

• None of the above.
• A balanced chemical equation follows the law of conservation of mass.
• The amount of limiting reagent present at the start of a reaction determines the theoretical yield of the reaction.
• A limiting reagent is the reactant that is used up first in a chemical reaction.

He was the first to formulate a concise definition of thermodynamics in 1854 which stated, "Thermo-dynamics is the subject of the relation of heat to forces acting between contiguous parts of bodies, and the relation of heat to electrical agency.

• Julius Robert von Mayer
• Nicolas Leonard SadiCarno
• Lord Kelvin (William Thomson)
• Rudolf Julius Emmanuel Clausius

According to the kinetic molecular theory, average kinetic energy of gas molecules is proportional to absolute temperature. At any given temperature, gas molecules have exactly similar average kinetic energy.

• True
• False

The lack of molecules above the surface of liquids causes them to tighten and form an elastic-like film.

• True
• False

Increasing the temperature also speeds up the reaction, hence, increasing the rate constants

• True
• False

When ΔS > 0 and ΔH > 0, the process will be ___________________ at high temperatures.

• None of the above
• Hard to tell
• Spontaneous
• Non-spontaneous

Which of the following rules is true with regards to assigning maximum number of electrons to orbitals (given n)?

• The principal quantum number No also dictates the number of subshells (two values of l)
• The number of orbitals is determined by the angular quantum number (l), computed as 2l + 1.
• None of the above
• All of the above

During a chemical reaction, the concentration of the reacting species increase over time while it is being consumed.

• True
• False

Which of the following are correct match of molecular and empirical formula?

• Carbon dioxide – CO2 / CO2
• Benzene – C6H6 / CH
• All of the above
• Phosphorus oxide – P4O8 / P2O4

Molecules in gases, under normal conditions, is observed to:

• All of the choices
• Exert great attractive forces together
• Have no great interaction between them
• Repel each other

Charle's Law states that at a constant pressure, the volume of a fixed amount of gas is inversely proportional to its absolute temperature

• True
• False

Among the states of matter it has the lowest entropy.

• Liquid
• Solid
• None
• Gas

It is defined as the measurement of disorder or randomness within the system

• State of a system

The difference between the colligative properties of electrolyte and nonelectrolyte solutions is the breaking up of solute particles in a solution. This is quantified and added to computation of concentration units using the:

• None of the above
• London factor
• van't Hoff factor
• van der Waals factor

The -ium ending on the name of hydronium indicates that it is a cation from metal atoms.

• True
• False

Given the following equation, write and compute for the equilibrium constant expression:

• 16
• 8
• 5
• 10

At constant temperature and volume, the total pressure of a gas is ___________ proportional to the number of moles of gas present.

• Directly
• Inversely

Calculate the pH of the buffer solutions below:

• pH = 2
• pH = 3.5
• pH = 4.74
• pH = 5

If the percent yield of the reaction is only 85% using 100.0 kg of ammonia.

• 329.5 kg
• 170 kg
• 85 kg
• 659.1 kg

What can affect the viscosity of a certain liquid?

• Strength of intermolecular forces
• Temperature
• All of the above
• Shape of molecules

Which of the following rules is not true with regards to assigning maximum number of electrons to orbitals (given n)?

• No correct answer
• The principal quantum number No also dictates the number of subshells (two values of l)
• Both of the statements are correct
• The number of orbitals is determined by the angular quantum number (l), computed as 2l + 1.

Dalton's law of partial pressure states that constant _____________ and volume, the total pressure of a gas is directly proportional to the number of moles of gas present.

• pressure
• temperature
• any of the given choices is correct
• distance

The freezing-point temperature of a solution is lower as compared to its pure solvent.

• True
• False

How many significant figures are in 5.070 x 103 g?

• 2
• 4
• 5
• 3

Why can glass be filled slightly above the rim with water without overflowing?

• Because of the water's temperature
• Because of surface tension
• Because of nonpolar molecules
• Because of atmospheric pressure

Elements can be decomposed into smaller substances.

• True
• False

During a chemical reaction, what happens to the concentration of the reactants?

• linearly increases
• nothing happens
• decreases
• exponentially increases

Dalton's law of partial pressure states that constant temperature and volume, the total pressure of a gas is ____________ proportional to the number of moles of gas present.

• inversely
• sometimes inversely, sometimes directly
• directly

Colligative properties depend on the nature of the substances in a solution.

• True
• False

Which of the following statement is true regarding Gas Laws?

• Boyle's Law states that at a constant temperature, the volume of a fixed amount of gas is inversely proportional to its pressure
• Charle's Law states that at constant temperature and pressure, volume of gas is directly proportional to the number of moles of gas present
• All of the above
• Avogadro's law states that at constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute temperature

One mole of Phosphorus, with atomic mass of 30.97 amu, has greater number of atoms than one mole of Boron, with atomic mass of 10.81 amu.

• True
• False

What is the name of the compound that has 2 nitrogen and 4 oxygen?

• nitrogen tetroxide
• dinitrogen tetroxide
• binitrogen tetroxide
• nitrogen (II) oxide

Valence electrons are also known as the innermost electrons.

• True
• False

The difference between the mass number and the atomic number equals the number of ________________ in an atom.

• Protons
• Neutrons
• Electrons

How does temperature affect rate constants?

• Increasing the temperature also speeds up the reaction, hence, decreasing the rate constants.
• Increasing the temperature also speeds up the reaction, hence, increasing the rate constants.
• Increasing the temperature also slows up the reaction, hence, increasing the rate constants.
• Increasing the temperature also slows up the reaction, hence, decreasing the rate constants.

The boiling-point temperature of a solution is higher than its pure solvent.

• True
• False

Which of the following is the reaction intermediate?

• NO2(g)
• O2(g)
• N2O2(g)
• NO(g)

Given the following concentrations for the decomposition of NO2 compute for the rate of the reaction in terms of the reactant, NO2.

• – 1.0 x 10-5mol L-1 s-1
• – 1.0 x 10-5mol Ls
• + 1.0 x 10-5mol L-1 s-1
• – 1.0 x 105mol L-1 s-1

The solubility of a sodium chloride in water at 25 degrees Celsius is 357g/L. What is the molar solubility of NaCl?

• 6.11M
• 4.67M
• 6.20M
• 5.3 M

What is the relationship between solubility of solids and temperature?

• Solubility of solids is not affected by temperature
• Solubility of solids decrease with temperature
• Solubility of solids increase with temperature.
• None of the choices

Which of the following has the highest ionization energy?

• Ga
• K
• Br
• Ca

Energy levels of orbitals determine the actual arrangement of electrons in atoms. Electrons will fill first the most stable orbitals.

• True
• False

This is a method used to distinguish a solution from a colloid, where light is beamed in a substance and observed if it would scatter due to dispersed particles observable in a colloid:

• Crystallization
• Van der Waals effect
• Effervescence
• Tyndall effect

A percent yield of 100% is impossible to attain in the laboratory.

• True
• False

It is a type of system that cannot transfer both mass and energy

• Isolated System

Determine the oxidation state of the mentioned element in the given compound :

• +6
• +2
• -5

What is defined as the amount of heat needed to raise the temperature of 1gram of the substance by 1K or 1C?

• Specific heat
• Heat capacity
• Kinetic energy
• Enthalpy

What is the mass percent of Hydrogen, H, in resveratrol?

• 5.26%
• 19.02%
• 5.31%
• 18.83%

A unit of measure of temperature based upon an absolute scale

• Kelvin
• Fahrenheit
• Celsius

The energy of a single photon is described as E = hv

• True
• False

What factor affect electronegativity?

• Electron affinity and Ionization energy
• Distance between nuclei
• Ionization energy
• Electron affinity

It is a state function defined as the ability to do work

• Energy

Solubilities of solids and gases affect differently with temperature.

• True
• False

Which of the following statements is true with regard to the relationship of lattice energy with the atoms' charges and the distance between them?

• Lattice energy is inversely proportional to the distance of separation between them.
• All of the above
• Lattice energy is inversely proportional to the product of their charges
• None of the above

How many grams are in 6.20 moles of Na?

• 22.99 grams
• 142.54 grams
• None of the above
• 3.71 grams

Which of the following has the greatest electron affinity?

• Be
• F
• Li
• B

Which of the following statement is true regarding Tyndall effect?

• It is a method used to distinguish a solution from a colloid, where light is beamed in a substance and observed if it would scatter due to dispersed particles observable in a colloid.
• None of the choices
• All of the choices
• It is possible to observe this with solutions

When does a chemical equilibrium occur?

• When free energy of the reaction is at its lowest possible value.
• When free energy of the reaction is at its highest possible value.
• When products are no longer produced.
• When reactants are no longer consumed.

Determine if the Starting Material underwent the following changes upon formation of their respective decay product nuclei:

• K-Capture
• Alpha emission
• Positron Emission
• Beta emission

Suppose synthesis of Al2O3 is done in the lab using 20.50 g of Al and excess of O2. Upon purification, 35.48 grams of Al2O3 is produced. What is the percent yield of Al2O3?

• 45.80%
• 91.58%
• 57.78%
• 22.90%

The number of electrons and protons are equal in number.

• True
• False

It would be impossible to perform work that results in an energy output greater than the energy input.

• True
• False

Chemical equilibrium is the state at which the free energy of the reaction is at its highest possible value.

• True
• False

What is an induced dipole moment?

• An induced dipole is a previous dipole molecule turned into a nonpolar one
• An induced dipole is caused when a nonpolar molecule creates a temporary dipole moment, due to a disturbance in the distribution of electrons.
• None of the choices
• An induced dipole molecule has a permanent positive and negative charge.

From the given pairs, determine which pair is the anode.

• Zn/ZnSO­4
• Cu/CuSO4

In the following chemical reaction, what can be done to maintain the forward reaction?

• Increase concentration of PCl5
• Decrease concentration of Cl2
• Decrease concentration of PCl3
• Increase concentration of PCl3

What traits can be observed with solids and liquids, due to little space in between molecules?

• Solids and liquids have observable shapes and volume
• Solids and liquids are expandable
• All of the above
• Solids and liquids have low density

It states that the entropy of a system approaches a constant value as the temperature approaches zero.

• Nernst's Theorem
• The Second Law of Thermodynamics
• The Law on Conservation of Energy
• Spontaneous Processes

In a balanced chemical equation, the number of atoms of an element on the left side is always equal to the number of atoms on the right side.

• True
• False

Determine each nuclear transmutation :

• K-Capture
• Beta emission
• Alpha emission
• Positron Emission

Convert 35.6 degrees Celsius to Fahrenheit

• 308.75 degrees Fahrenheit
• 69.1 degrees Fahrenheit
• 2 degrees Fahrenheit
• 96.1 degrees Fahrenheit

Which of the following statement is true regarding balancing chemical equations?

• Both of the given statements are correct
• No correct answer
• Balance first those elements that appear in only one reactant and one product. Then, balance elements that appear in more than one reactant and product.
• The common convention for balanced equations is to use the smallest whole numbers

Which of the following is NOT a type of concentration unit?

• Pressure
• Mole Fraction
• Molarity
• Molality

Which of the following concentration units is NOT independent of temperature?

• All of the choices
• Molality
• Molarity
• Percent by mass

Direction : Identify if the following elements are metal, non-metal or metalloids:

• Metalloids
• Metal
• Non-metal

Which of the following can increase the pressure of a gas?

• Lower velocity
• Bigger container
• Smaller number of molecules
• Smaller container

Why can't we write Lewis structures for lanthanides, actinides, and transition metals?

• None of the choices
• All of the choices
• Because of the number of electrons not equal to eight
• Because of their incompletely filled inner shells

Which of the following affects chemical equilibrium?

• Temperature
• Concentration
• Pressure
• All of the choices

Accuracy is a measure of how closely individual measurements are to the actual or true value, while precision refers as to how closely individual measurements are to one another.

• True
• False

Chemical equilibrium is the state in which there is no apparent change in the products and reactants over time, and the free energy of the reaction is at its lowest.

• True
• False

Henderson-Hasselbalch equation s the equation relating between pH and pKa.

• True
• False

A homogeneous catalysis occurs using a catalyst that has a different phase as the reacting molecules while a heterogeneous catalysis occurs when a catalyst has the same phase as the reactants.

• True
• False