Chapters 10, 11, 12 Physics

The charge on alkali metal ions is +2. -1. +1. -2.

+1.

The number of hydrogen atoms in a molecule of ammonium sulfide, (NH4)2S, is 6. 8. 4. 2.

8

The scientist whose experiments showed that tin upon heating combined with a gas from the air was Priestley. Stahl. Lavoisier. Becher.

Lavoisier.

An atom whose outer electron shell lacks one electron of being filled is an active metal. a halogen. an inert gas. an inactive metal.

a halogen.

The individual particles in a metal are held together as a result of the attraction of polar molecules. electron sharing between adjacent atoms. electron transfer between adjacent atoms. a sea of freely-moving electrons.

a sea of freely-moving electrons.

According to the periodic table, the chemical properties of the elements are periodic functions of their density. mass number. atomic number. atomic mass.

atomic number.

Most solids are polar. amorphous. crystalline. covalent

crystalline.

An example of slow oxidation is a lighted candle. a log burning in a fireplace. the rusting of iron. the lighting of a match.

the rusting of iron.

The speed of a chemical reaction is not affected by the concentration of reactants. the type of bond in reaction products. the surface area of the reactants. catalysts.

the type of bond in reaction products.

The mass of 1 mole of oxygen, O2, is 32g. The atomic mass of oxygen is 16 g. 32 u. 32 g. 16 u.

16 u.

The atomic mass of N is 14 u and that of Ca is 40 u. The proportion of N by mass in the compound Ca3N2is 40 percent. 81 percent. 19 percent. 35 percent.

19 percent.

The missing number in the equation 2HNO3+Ca(OH)2→Ca(NO3)2+( )H2O is 2. 3. 1. 4.

2

The number of moles of O2 needed to react with 10 moles of C2H2 in the reaction 2C2 H2 + 5O2 → 4CO2 + 2 H2O is 10. 5. 50. 25.

25.

Pure water has a pH of 10. 7. 1. 0.

7.

The scientist who first established the relative masses of different elements was Priestley. Mendeleev. Maxwell. Dalton.

Dalton.

The fundamental reaction of neutralization is H++H2O→H3O+ H2O→H++OH- H2O+H2O→H3O++OH- H++OH-→H2O

H++OH-→H2O

The symbol of the hydronium ion is H3O-. OH-. OH+. H3O+.

H3O+.

Which of the following would you expect to be a strong electrolyte in solution? soap AgCl NaCl acetic acid

NaCl

The ion of the hydroxide group has the symbol OH. OH-. OH+. H2O-.

OH-.

The symbol of the hydroxide ion is OH-. OH+. H3O+. H3O-.

OH-.

One mole of which of the following compounds contains the largest number of fluorine atoms? HF SF2 XeF6 BF3

XeF6

In a covalent compound electrons are shifted from one atom to another. there must be at least one carbon atom. adjacent atoms share electron pairs. only atoms of the same element are present.

adjacent atoms share electron pairs.

A solid whose particles are irregularly arranged with no definite pattern is said to be a van der Waals solid. nonpolar. unsaturated. amorphous.

amorphous.

An atom whose outer electron shell is filled is an active metal. an inert gas. a halogen. an inactive metal.

an inert gas.

The most active of the following nonmetals is oxygen. chlorine. carbon. helium.

chlorine.

The strongest bonds are metallic. van der Waals. ionic. covalent.

covalent.

The individual particles in a covalent solid are held together as a result of the attraction of polar molecules. a gas of freely-moving electrons. electron sharing between adjacent atoms. electron transfer between adjacent atoms.

electron sharing between adjacent atoms.

The individual particles in an ionic solid are held together as a result of the attraction of polar molecules. electron transfer between adjacent molecules. a sea of freely-moving electrons. electron sharing between adjacent atoms.

electron transfer between adjacent molecules.

Oxidation-reduction reactions involve the transfer between the reacting substances of O2- ions. electrons. O2 molecules. H+ ions.

electrons.

Chemical reactions that give off energy are called oxidation-reduction. exothermic. endothermic. activated.

exothermic.

A vertical column in the periodic table is called a subshell. group. shell. period.

group

Carbon has properties no other element has. is a typical metal. has properties intermediate between those of metals and nonmetals. is a typical nonmetal.

has properties intermediate between those of metals and nonmetals.

Polar molecules behave as though they have a negative charge at both ends. have a positive charge at one end and a negative charge at the other. have a positive charge at both ends. contain tiny magnets.

have a positive charge at one end and a negative charge at the other.

Elements with similar properties (other than atomic mass) exist in the same physical state (solid, liquid, or gas). have similar electron configurations. have the same number of neutrons in their nuclei. occupy the same period of the periodic table.

have similar electron configurations.

The least active of the following nonmetals is oxygen. carbon. chlorine. helium.

helium.

The most abundant element in the universe is hydrogen. oxygen. helium. carbon.

hydrogen.

An example of a molecular solid is tin. ice. diamond. table salt

ice.

Dissolving an electrolyte in water results in the formation of ions. polar molecules. a precipitate. covalent molecules.

ions.

The decomposition of an unstable compound usually occurs only at low temperatures. requires a catalyst to occur. is exothermic. is endothermic.

is exothermic.

Bases do not taste bitter. liberate H2 when mixed with an active metal. turn red litmus to blue. produce OH- ions in water solution.

liberate H2 when mixed with an active metal.

Acids do not combine with active metals to give off H2. neutralize bases. liberate OH- ions when dissolved in water. taste sour.

liberate OH- ions when dissolved in water.

The largest number of elements are classed as liquids. nonmetals. metals. inert gases.

metals

When a strong acid is added to water, more of it forms hydroxide ions than in the case of a weak acid. more of it dissociates than in the case of a weak acid. less of it forms hydronium ions than in the case of a weak acid. more of it dissolves than in the case of a weak acid.

more of it dissociates than in the case of a weak acid.

When 1 g of a metal is oxidized, the resulting oxide has a mass that is more than 1 g. equal to 1 g. less than 1 g. Any of the choices, depending on the metal.

more than 1 g.

When equivalent amounts of a strong acid and a strong base react, the resulting solution is pure water. neutral. acidic. basic.

neutral.

An example of an exothermic process is the electrolysis of water. neutralization of an acid by a base. dissociation of a salt in water solution. melting of ice.

neutralization of an acid by a base.

A horizontal row in the periodic table is called a period. subshell. group. shell.

period

Ionic crystals dissolve only in liquids that are supersaturated. nonpolar. polar. saturated.

polar

The most active of the following metals is lead. copper. potassium. gold.

potassium

The energy liberated in a chemical reaction comes from the equilibrium energy of atomic electrons. kinetic energy of atomic electrons. potential energy of atomic electrons. activation energy of atomic electrons.

potential energy of atomic electrons.

When a substance gains electrons in a chemical reaction, the substance is said to be activated. oxidized. dissociated. reduced.

reduced.

A chemical equilibrium occurs when the number of molecules of the products equals the number of molecules of the reactants. speed of the forward reaction equals the speed of the reverse reaction. concentration of the products equals the concentration of the reactants. mass of the products equals the mass of the reactants.

speed of the forward reaction equals the speed of the reverse reaction.

The atomic mass of an element is the average atomic number of its isotopes according to their proportions in nature. the average mass number of its isotopes according to their proportions in nature. the average atomic mass of its isotopes according to their proportions in nature. the atomic mass of its most abundant isotopes.

the average mass number of its isotopes according to their proportions in nature.

The statement that the elements in a given compound are always combined in the same proportions by mass is known as the law of definite proportions. the periodic law. the law of conservation of mass. Dalton's law.

the law of definite proportions.

The weakest bonds are van der Waals. covalent. ionic. metallic.

van der Waals.