Reference no: EM131940951

1.Which phase of matter is made up of particles that are packed closely together, with both a definite shape and a definite volume?

A.Gas

B.Liquid

C.Plasma

D.Solid

2.Which of the following describes what occurs as a solid becomes a liquid?

A.A chemical change occurs; the particles of the solid vibrate more slowly and their kinetic energy decreases.

B.A chemical change occurs; the particles of the solid vibrate faster and their kinetic energy increases.

C.A physical change occurs; the particles of the solid vibrate more slowly and their kinetic energy decreases.

D.A physical change occurs; the particles of the solid vibrate faster and their kinetic energy increases.

3.A sample of gas has a volume of 2.4 L and a pressure of 1.2 atm. What would the pressure of the same gas sample be if the volume is reduced to 1.8 L at a constant temperature?

A.0.90 atm

B.1.6 atm

C.5.2 atm

D.3.6 atm

4.If 2.0 moles of O2 gas occupy a volume of 56 liters at a temperature of 298 K, what is the pressure of the gas, in atmospheres (atm)?

A.0.073 atm

B.0.87 atm

C.1.1 atm

D.1.7 atm

5.Which of the following explains why the substances cannot dissolve in water?

A.Sugar, because it is an ionic substance

B.Oil, because it is a nonpolar covalent substance

C.Sugar, because it is a nonpolar covalent substance

D.Oil, because it is an ionic substance

6.How would a system in which both matter and energy are exchanged freely between the system and the surroundings be classified?

A.An open system

B.An isolated system

C.A closed system

D.An integrated system

7.Hydrogen peroxide will decompose if the bottle is left open, and the resulting release of energy will heat up the solution. Which of the following best describes this type of reaction?

A.Endothermic

B.Exothermic

C.Combustion

D.Synthesis

8.On a potential energy diagram, what type of reaction will always have the reactants at a higher potential energy than the products?

A.Exothermic reaction

B.Endothermic reaction

C.Synthesis reaction

D.Single replacement reaction

9.According to the collision theory and the model created to explain the collision theory, what two factors must be satisfied for a given collision to be successful and result in the production of products?

A.Correct molecular shape and momentum

B.Correct position and maximum potential

C.Correct density and threshold velocity

D.Correct orientation and sufficient energy

10.Which of the following is not true of acids?

A.Acids are corrosive.

B.Acids feel slippery.

C.Acids have a sour taste.

D.Acids have more hydronium ions than hydroxide ions.

11.Which of the following is the salt in the Brønsted-Lowry neutralization reaction?

HBr + NaOH H2O + NaBr

A.HBr

B.NaOH

C.H2O

D.NaBr

12.Which of the following pH levels would be the most acidic?

A.pH 2.0

B.pH 5.0

C.pH 8.0

D.pH 12.0

13.Which answer describes a chemical reaction in equilibrium?

A.The reactants are all used up.

B.All the product is formed.

C.The forward and reverse reactions have ceased.

D.The forward and reverse reaction rates are the same.

14.Which of the following is not a result when a change to an equilibrium system is applied?

A.Increasing the rate of the forward reaction will cause a shift to the left.

B.Increasing the rate of the reverse reaction will cause a shift to the left.

C.Decreasing the rate of the forward reaction will cause a shift to the left.

D.Decreasing the rate of the reverse reaction will cause a shift to the right.

15.In the chemical reaction shown below, which element was oxidized?

2K + Cl2 2KCl

A.K, because it lost one electron

B.K, because it gained one electron

C.Cl, because it lost one electron

D.Cl, because it gained one electron

16.Which of the following types of radiation can be shielded by a piece of paper or fabric?

A.Alpha rays

B.Beta rays

C.Gamma rays

D.Proton rays

17.Which statement is not true regarding nuclear reactions?

A.Nuclear reactions involve a change in an atom's nucleus.

B.Alpha, beta, and gamma are types of radiation.

C.Nuclear reactions involve breaking and forming covalent bonds.

D.Radioactive elements have unstable nuclei.

18.Which of the following describes nuclear fission?

A.it requires extremely high temperatures to begin the reaction.

B.It involves two atoms combining into one larger atom.

C.It involves two atoms bonding together with shared electrons.

D.It involves one atom splitting into two or more smaller atoms.

19.Which of the following best describes nuclear fusion?

A.It fuels nuclear power plants.

B.It involves the splitting of one atom into two smaller atoms.

C.It involves the combining of two atoms into one larger atom.

D.Its chain reactions can be initiated by electrons.

20.How many valence electrons do the alkali metals have? (2 points)

A.1

B.2

C.7

D.8

21.How many valence electrons do most of the noble gases have? (2 points)

A.1

B.2

C.7

D.8

22.How many valence electrons do the halogens have? (2 points)

A.1

B.2

C.7

D.8

23.How many valence electrons do the alkaline-earth elements have? (2 points)

A.1

B.2

C.7

D.8

24.What are properties of the group of elements on the periodic table that have seven valence electrons? (2 points)

A.High reactivity, metallic

B.High reactivity, nonmetallic

C.Low reactivity, metallic

D.Low reactivity, nonmetallic

25.What are properties of the group of elements on the periodic table that have just one valence electron? (2 points)

A.Gas at room temperature

B.Soft and highly reactive

C.Unstable and radioactive

D.Very low reactivity

26.Which statement describes the properties of both elements that have just one valence electron and elements that have seven valence electrons? (2 points)

A.They are highly reactive.

B.They are gases at room temperature.

C.They exist in nature as pure elements.

D.They easily give up an electron.

27.What is the trend in effective nuclear charge for elements on the periodic table?

A.It decreases across a period but is constant down a group.

B.It increases across a period but is constant down a group.

C.It is constant across a period but decreases down a group.

D.It is constant across a period but increases down a group.

28.On the periodic table, the number of valence electrons in atoms increases left to right across a period. What effect does this have on the ionic radii of the elements?

A.It decreases across cations and decreases across anions.

B.It decreases across cations and increases across anions.

C.It increases across cations and decreases across anions.

D.It increases across cations and increases across anions.

29.How does the atomic radius change as you move down a group on the periodic table?

A.It decreases because additional valence electrons are farther from the nucleus.

B.It decreases because additional valence electrons experience more shielding.

C.It increases because additional valence electrons are farther from the nucleus.

D.It increases because additional valence electrons experience more shielding.

29.What is the trend in electronegativity for elements on the periodic table?

A.It decreases across a period and increases down a group.

B.It decreases across a period and decreases down a group.

C.It increases across a period and increases down a group.

D.It increases across a period and decreases down a group.

30.Which statement describes the trend in first ionization energy for elements on the periodic table?

A.It generally decreases down a group because valence electrons are farther from the nucleus.

B.It generally decreases across a period because effective nuclear charge decreases.

C.It generally increases down a group because valence electrons are farther from the nucleus.

D.It generally increases across a period because effective nuclear charge decreases.