semester a final review

Semester A

Final Review

Rules

Answer in your own poll pod.

How are science and technology related?

A. Technology is a branch of natural

science.

B. Science is a branch of technology.

C. Advances in science may lead to

advances in technology and vice versa.

D. Science and technology are not related.

Why are scientific models important?

A. They prove scientific theories.

B. They help visualize things that are very

complex, very large, or very small.

C. They make it harder to understand

things.

D. They never change.

Timers at a swim meet used four

different clocks to time an event. Which

recorded time is the most precise?

A. 55 s

B. 55.2 s

C. 55.25 s

D. 55.254 s

If the relationship between the manipulated variable

and the responding variable is a direct proportion,

what will a line graph of this relationship look like?

A. a straight line

B. a curved line

C. a jagged line

D. none of the above

Which of the following is NOT a pure

substance?

A. milk

B. oxygen

C. water

D. carbon dioxide

Water is a compound

because it …

A. can be broken down into simpler

substances.

B. always has two hydrogen atoms for

each oxygen atom.

C. is made of water atoms joined together.

D. both a and b

Which of the following is a

heterogeneous mixture?

A. water in a swimming pool

B. sugar water

C. a jar of mixed nuts

D. stainless steel

Filtration can be used to

separate mixtures based on …

A. their boiling points.

B. their densities.

C. their melting points.

D. the size of their particles.


physical change?

A. sawing a piece of wood in half

B. burning a piece of wood

C. rust forming on an iron fence

D. a copper roof changing color from red

to green


clue that a chemical change has

occurred?

A. Iron changes color when heated.

B. Gas bubbles form in boiling water.

C. Balls of wax form when melted wax is

poured into ice water.

D. A gas forms when vinegar and baking

soda are mixed.

Forces of attraction limit the

motion of particles most in

A. a solid.

B. a liquid.

C. a gas.

D. both b and c

Which of the following will cause a

decrease in gas pressure in a

closed container?

A. lowering the temperature

B. reducing the volume

C. adding more gas

D. both a and b

If a solid piece of naphthalene is heated and

remains at 80°C until it is completely melted,

you know that 80ºC is the …

A. freezing point of naphthalene.

B. melting point of naphthalene.

C. boiling point of naphthalene.

D. both a and b

During which phase change does

the arrangement of water

molecules become more orderly?

A. melting

B. freezing

C. boiling

D. condensing

The phase change in which a substance

changes from a solid to a gas or vapor

without changing to a liquid first is…

A. sublimation.

B. deposition.

C. vaporization.

D. melting.

Which phase change is an

endothermic change?

A. condensation

B. vaporization

C. deposition

D. freezing

How was Bohr’s atomic model

similar to Rutherford’s model?

A. It assigned energy levels to electrons.

B. It described electron position in terms of

the electron cloud model.

C. It described how electrons gain or lose

energy.

D. It described a nucleus surrounded by a

large volume of space.

What is the difference between

an atom in the ground state and

an atom in an excited state?

A. The atom in the ground state has less energy and is less stable than the atom in an excited state.

B. The atom in an excited state has one fewer electron than the atom in the ground state.

C. The atom in an excited state has more energy and is less stable than the atom in the ground state.

D. The atom in an excited state has one more electron than the atom in the ground state.

The usefulness of Mendeleev’s

periodic table was confirmed by…

A. the discovery of subatomic particles.

B. its immediate acceptance by other

scientists.

C. the discovery of elements with predicted

properties.

D. the discovery of the nucleus.

The atomic mass of an

element is …

A. the sum of the protons and neutrons in

one atom of the element.

B. twice the number of protons in one

atom of the element.

C. a ratio based on the mass of a carbon-

12 atom.

D. a weighted average of the masses of an

element’s isotopes.

Which general statement

does NOT apply to metals?

A. Most metals are ductile.

B. Most metals are malleable.

C. Most metals are brittle.

D. Most metals are good conductors of

electric current.

Among the alkali metals, the

tendency to react with other

substances …

A. does not vary among the members of

the group.

B. increases from top to bottom within the

group.

C. varies in an unpredictable way within

the group.

D. decreases from top to bottom within the

group.

Study the electron dot diagrams for lithium,

carbon, fluorine, and neon in the figure.

Choose the statement that correctly identifies

the most stable of the elements.

A. Lithium is the most stable element because it has to lose only one electron to achieve a stable configuration.

B. Carbon is the most stable element because it can form four bonds.

C. Fluorine is the most stable element because it has to gain only one electron to achieve a stable configuration.

D. Neon is the most stable element because its highest occupied energy level is filled.

The formation of an ionic

bond involves the …

A. transfer of electrons.

B. transfer of neutrons.

C. transfer of protons.

D. sharing of electrons.

In a polar covalent bond, …

A. electrons are shared equally between

atoms.

B. a cation is bonded to an anion.

C. electrons are transferred between

atoms.

D. electrons are not shared equally

between atoms.

Beryllium, Be, and chlorine, Cl, form a binary

ionic compound with a one-to-two ratio of

beryllium ions to chloride ions. The formula for

the compound is …

A. Be2Cl.

B. Be2Cl.

C. BeCl2.

D. Be2Cl2.

When magnesium carbonate, MgCO2, reacts with nitric acid,

HNO3, magnesium nitrate and carbonic acid form. Carbonic

acid then breaks down into water and carbon dioxide. Which

two types of reactions take place in this process?

A. synthesis and decomposition

B. single-replacement and combustion

C. double-replacement and

decomposition

D. double-replacement and combustion

In terms of energy, how would you

classify the following chemical

reaction?

2Cu + O2 2CuO + 315 kJ

A. endothermic

B. exothermic

C. both endothermic and exothermic

D. neither endothermic nor exothermic

A log is burning in a fireplace. If the amount of

oxygen reaching the log is decreased, which

of the following statements is true?

A. The reaction rate increases.

B. The reaction rate decreases.

C. The reaction rate remains the same.

D. The reaction rate depends only on the

temperature.

A student dissolved equal amounts of salt in

equal amounts of warm water, room-

temperature water, and ice water. Which of

the following is true?

A. The salt dissolved most quickly in the

warm water.

B. The salt dissolved most quickly in the

room-temperature water.

C. The salt dissolved most quickly in the ice

water.


A solution that contains more solute

than it would normally hold at that

temperature is said to be…

A. saturated.

B. unsaturated.

C. supersaturated.

D. concentrated.

Which of the following is NOT a

property of an acid?

A. tastes sour

B. usually reacts with a metal

C. changes the color of an indicator

D. feels slippery

A base is defined as a

compound that produces …

A. hydroxide ions in solution.

B. hydrogen ions in solution.

C. hydronium ions in solution.

D. sodium ions in solution.

A small amount of acid is added

to a buffer solution. The pH of the

solution will …

A. increase.

B. decrease.

C. stay about the same.

D. become neutral.

Uranium-238 undergoes alpha

decay. Therefore, uranium-238

will…

A. remain stable.

B. change into a different element

altogether.

C. emit neutral particles and no energy.


What type of radiation is emitted

when polonium-212 forms lead-

208?

A. an alpha particle

B. a beta particle

C. gamma radiation

D. all of the above

Transmutation involves…

A. nuclear change.

B. chemical change.

C. both a nuclear change and a chemical

change.

D. neither a nuclear nor a chemical

change.

During nuclear fission, great

amounts of energy are produced

from…

A. very small amounts of mass.

B. tremendous amounts of mass.

C. a series of chemical reactions.

D. particle accelerators.

Which of the following conversion

factors would you use to change 18

kilometers to meters?

A. 1000 m/1 km

B. 1 km/1000 m

C. 100 m/1 km

D. 1 km/100 m

According to John Dalton’s

observations, when elements

combine in a compound, …

A. the ratio of their masses is always the

same.

B. each element contributes an equal

number of atoms.

C. their volumes are always equal.

D. their masses are always equal.

Which of the following provides

the best analogy for an electron in

an atomic orbital?

A. a bee moving from flower to flower in a

garden

B. a bird resting on a tree branch

C. an ant crawling on the surface of a leaf

D. a bee trying to escape from a closed jar

The tendency of an element

to react is closely related to…

A. its atomic mass.

B. attractions between its atoms.

C. the number of valence electrons in

atoms of the element.

D. the ratio of protons to neutrons in atoms

of the element.

If a gas has a volume of 1 L at a pressure of 270 kPa, what volume will it have when the pressure is increased

to 540 kPa? Assume the temperature and number of

particles are constant.

How many grams of O2 are in

5.0 moles of the oxygen gas?

What are the products of a

neutralization reaction?

Sodium reacts with chlorine gas to form sodium chloride. Write a balanced chemical equation for the

reaction, and find the mass of chlorine gas that will

react with 96.6 g of sodium.

After 15 minutes, 30 g of a sample of

polonium-218 remain unchanged. If the

original sample had a mass of 960 g, what is

the half-life of polonium-218?

Explain the difference between a

physical equilibrium and a

chemical equilibrium.

Suppose you want to separate the leaves, acorns, and twigs

from a pile of soil. Filtration and distillation are two processes

of separating mixtures. Explain which process you would use

and why.

What is the charge on the subatomic particles represented in Figure 4-3? Assuming all the particles in

the nucleus are visible, what are the atomic and mass

numbers of the atom shown?