Ch. 7 Chemistry

All the elements in group 8A are gases at room temperature. Of all the groups in the periodic table, only group ____ contains examples of elements that are gas, liquid, and solid at room temperature. a. 7A b. 1A c. 2A d. 5A e. 6A

a. 7A

Of the elements below, ____ has the highest melting point. a. Fe b. K c. Ba d. Na e. Ca

a. Fe

The substance ____ is always produced when an active metal reacts with water. a. H2 b. H2O c. NaOH d. CO2 e. O2

a. H2

This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ____. a. Na b. Be c. Rb d. Ca e. Fr

a. Na

Which of the following has the largest second ionization energy? a. Na b. Mg c. Si d. P e. Al

a. Na

Of the elements below, ____ is the least metallic. a. Ne b. S c. Cl d. O e. F

a. Ne

Which one of the following elements has an allotrope that is produced in the upper atmosphere by lightning? a. O b. He c. S d. N e. Cl

a. O

In which set of elements would all members be expected to have very similar chemical properties? a. O, S, Se b. Na, Mg, K c. N, O, F d. Ne, Na, Mg e. S, Se, Si

a. O, S, Se

In which of the following atoms is the 3s orbital closest to the nucleus? a. Po b. Te c. Se d. P e. S

a. Po

When two elements combine to form a compound, the greater the difference in metallic character between the two elements, the greater the likelihood that the compound will be ____. a. a solid at room temperature b. a liquid at room temperature c. nonmetallic d. metallic e. a gas at room temperature

a. a solid at room temperature

Which of the following is not a characteristic of metals? a. acidic oxides b. low ionization energies c. These are all characteristics of metals. d. ductility e. malleability

a. acidic oxides

Elements in the modern version of the periodic table are arranged in order of increasing ____. a. atomic number b. atomic mass c. oxidation number d. number of isotopes e. average atomic mass

a. atomic number

In general, as you go across a period in the periodic table from left to right: (1) the atomic radius ____; (2) the electron affinity becomes ____ negative; and (3) the first ionization energy ____. a. decreases, increasingly, increases b. increases, increasingly, increases c. increases, increasingly, decreases d. decreases, decreasingly, increases e. decreases, increasingly, decreases

a. decreases, increasingly, increases

Alkaline earth metals ____. a. form basic oxides b. form halides with the formula MX c. exist as triatomic molecules d. form monoanions e. have the smallest atomic radius in a given period

a. form basic oxides

The alkali metal that is naturally radioactive is ____. a. francium b. lithium c. cesium d. rubidium e. sodium

a. francium

The effective nuclear charge of an atom is primarily affected by ____. a. inner electrons b. electron distribution c. orbital radial probability d. outer electrons e. nuclear charge

a. inner electrons

In nature, sulfur is most commonly found in ____. a. metal sulfides b. H2S c. pure elemental sulfur d. sulfur oxides e. sulfuric acid

a. metal sulfides

Which of the following traits characterizes the alkali metals? a. the lowest first ionization energies in a period b. the smallest atomic radius in a period c. existence as diatomic molecules d. very high melting point e. formation of dianions

a. the lowest first ionization energies in a period

The atomic radius of main-group elements generally increases down a group because ____. a. the principal quantum number of the valence orbitals increases. b. effective nuclear charge increases down a group c. both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases d. effective nuclear charge zigzags down a group e. effective nuclear charge decreases down a group

a. the principal quantum number of the valence orbitals increases.

The electron configuration of the atom that is expected to have a positive electron affinity is ____. a. (iii) b. (ii) c. (i) d. (v) e. (iv)

b. (ii)

A tin atom has 50 electrons. Electrons in the ____ subshell experience the lowest effective nuclear charge. a. 3d b. 5p c. 3p d. 1s e. 5s

b. 5p

Ca reacts with element X to form an ionic compound with the formula CaX. Al will react with X to form ____. a. AlX b. Al2X3 c. AlX2 d. Al3X e. Al3X2

b. Al2X3

____ have the lowest first ionization energies of the groups listed. a. Alkaline earth metals b. Alkali metals c. Transition elements d. Halogens e. Noble gases

b. Alkali metals

In which set of elements would all members be expected to have very similar chemical properties? a. Cl, Br, Na b. Br, I, At c. Ne, Na, Mg d. Si, As, Te e. P, Se, I

b. Br, I, At

Of the following oxides, ____ is the most acidic. a. Li2O b. CO2 c. Al2O3 d. CaO e. Na2O

b. CO2

Which one of the following compounds would produce an acidic solution when dissolved in water? a. SrO b. CO2 c. CaO d. Na2O e. MgO

b. CO2

Which equation correctly represents the first ionization of copper? a. Cu2+(g) ® Cu3+(g) + e- b. Cu(g) ® Cu+(g) + e- c. Cu+(g) ® Cu2+(g) + e- d. Cu(g) ® Cu-(g) + e- e. Cu+(g) + e-® Cu(g)

b. Cu(g) ® Cu+(g) + e-

Which element is solid at room temperature? a. Cl2 b. I2 c. Br2 d. F2 e. H2

b. I2

An alkaline earth metal forms a compound with oxygen with the formula ____. (The symbol M represents any one of the alkaline earth metals.) a. M2O b. MO c. MO3 d. MO2 e. M2O2

b. MO

The ion with the largest diameter is ____. a. Te2- b. Po2- c. Se2- d. S2- e. O2-

b. Po2-

Which one of the following compounds produces a basic solution when dissolved in water? a. OBr2 b. Rb2O c. ZnCl2 d. N2 e. SO2

b. Rb2O

____ is isoelectronic with krypton. a. Te2- b. Se2- c. Br d. Se3- e. Se2+

b. Se2-

The list that correctly indicates the order of metallic character is ____. a. Li > Na > K b. Sr > Ca > Mg c. C > Ge > Si d. F > Cl > Br e. O > Se > S

b. Sr > Ca > Mg

The ____ have the most negative electron affinities. a. alkali metals b. halogens c. chalcogens d. transition metals e. alkaline earth metals

b. halogens

In nature, sulfur is most commonly found in ____. a. sulfuric acid b. metal sulfides c. pure elemental sulfur d. sulfur oxides e. H2S

b. metal sulfides

Screening of the nuclear charge by core electrons in atoms is ____. a. both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group b. more efficient than that by valence electrons c. essentially identical to that by valence electrons d. less efficient than that by valence electrons e. responsible for a general decrease in atomic radius going down a group

b. more efficient than that by valence electrons

Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ____ in Ar. a. paramagnetism b. nuclear charge c. Hund's rule d. azimuthal quantum number e. diamagnetism

b. nuclear charge

Which of the following traits characterizes the alkali metals? a. the smallest atomic radius in a period b. the lowest first ionization energies in a period c. very high melting point d. existence as diatomic molecules e. formation of dianions

b. the lowest first ionization energies in a period

The electron configuration of the atom with the most negative electron affinity is ____. a. (iii) b. (ii) c. (v) d. (iv) e. (i)

c. (v)

Hydrogen is unique among the elements because ____. 1. It has only one valence electron. 2. It is the only element that can emit an atomic spectrum. 3. Its electron is not at all shielded from its nucleus. 4. It is the lightest element. 5. It is the only element to exist at room temperature as a diatomic gas. a. 1, 2, 3, 4 b. 1, 2, 3, 4, 5 c. 3, 4 d. 2, 3, 4 e. 1, 3, 4

c. 3, 4

Of the following species, ____ has the largest radius. a. Kr b. Sr2+ c. Br- d. Rb+ e. Ar

c. Br-

Which ion below has the largest radius? a. Cl- b. K+ c. Br- d. Na+ e. F-

c. Br-

Which equation correctly represents the electron affinity of calcium? a. Ca (g) ® Ca- (g) + e- b. Ca (g) ® Ca+ (g) + e- c. Ca (g) + e- ® Ca- (g) d. Ca- (g) ® Ca (g) + e- e. Ca+ (g) + e- ® Ca (g)

c. Ca (g) + e- ® Ca- (g)

The alkali metal that is used to treat manic-depressive illness is ____. a. Na b. K c. Li d. Rb e. Cs

c. Li

____ is isoelectronic with argon, and ____ is isoelectronic with neon. a. N3-, P3- b. P2-, N2- c. P3-, N3- d. P, N e. P3+, N3+

c. P3-, N3-

Of the following elements, ____ has the most negative electron affinity. a. Na b. K c. S d. B e. O

c. S

Alkali metals tend to be more reactive than alkaline earth metals because ____. a. Alkali metals are not more reactive than alkaline earth metals. b. alkali metals have lower densities c. alkali metals have lower ionization energies d. alkali metals have lower melting points e. alkali metals have greater electron affinities

c. alkali metals have lower ionization energies

Oxides of most nonmetals combine with water to form ____. a. hydrogen gas b. a base c. an acid d. water e. water and a salt

c. an acid

Most of the elements on the periodic table are ____. a. metalloids b. liquids c. metals d. gases e. nonmetals

c. metals

In nature, the noble gases exist as ____. a. alkali metal salts b. the sulfides c. monatomic gaseous atoms d. the gaseous fluorides e. solids in rocks and in minerals

c. monatomic gaseous atoms

Nonmetals can be ____ at room temperature. a. solid or liquid b. liquid only c. solid, liquid, or gas d. solid only e. liquid or gas

c. solid, liquid, or gas

The electron configuration belonging to the atom with the highest second ionization energy is ____. a. (iii) b. (v) c. (iv) d. (i) e. (ii)

d. (i)

Consider the general valence electron configuration of ns2np5 and the following statements: (i) Elements with this electron configuration are expected to form -1 anions. (ii) Elements with this electron configuration are expected to have large positive electron affinities. (iii) Elements with this electron configuration are nonmetals. (iv) Elements with this electron configuration form acidic oxides. Which statements are true? a. (i) and (ii) b. (i), (ii), and (iii) c. (ii) and (iii) d. (i), (iii,) and (iv) e. All statements are true.

d. (i), (iii,) and (iv)

The most common sulfur ion has a charge of ____. a. Sulfur does not form ions. b. 6+ c. 1- d. 2- e. 4+

d. 2-

2F2 (g) + 2H2O (l) → ____ a. 2F- (aq) + 2H+ (aq) + H2O2 (aq) b. 4HF (aq) + 2O2- (aq) c. 2HF2 (aq) + 2OH- (aq) d. 4HF (aq) + O2 (g) e. 2HF (aq) + 2HFO (aq)

d. 4HF (aq) + O2 (g)

Which ion below has the largest radius? a. F- b. K+ c. Na+ d. Br- e. Cl-

d. Br-

____ is isoelectronic with argon. a. K- b. P4- c. F- d. Cl- e. Ca

d. Cl-

____ is isoelectronic with scandium. a. Mn4- b. K+ c. Mn5+ d. Cr3+ e. Mn

d. Cr3+

Which of the following statements is not true for oxygen? a. The most stable allotrope of oxygen is O2. b. Oxygen is a colorless gas at room temperature. c. The chemical formula of ozone is O3. d. Dry air is about 79% oxygen. e. Oxygen forms peroxide and superoxide anions.

d. Dry air is about 79% oxygen.

Cl2 (g) + H2O (l) → ____ a. 2HCl (aq) + O2- (g) b. 2HCl (aq) + O2 (g) c. 2Cl- (aq) + H2O (l) d. HCl (aq) + HOCl (aq) e. Cl2 (aq) + H2O (l)

d. HCl (aq) + HOCl (aq)

The first noble gas to be incorporated into a compound was ____. a. Ar b. Ne c. Kr d. Xe e. He

d. Xe

In the generation of most anions, the energy change (kJ/mol) that ____ an electron is ____. a. removes, positive b. adds, positive c. removes, negative d. adds, negative e. None of the above is correct.

d. adds, negative

The reaction of alkali metals with oxygen produce ____. a. oxides b. peroxides c. superoxides d. all of the above e. none of the above

d. all of the above

The first ionization energies of the elements ____ as you go from left to right across a period of the periodic table, and ____ as you go from the bottom to the top of a group in the table. a. The first ionization energies of the elements are completely unpredictable. b. decrease, increase c. decrease, decrease d. increase, increase e. increase, decrease

d. increase, increase

The oxide of which element below can react with hydrochloric acid? a. selenium b. carbon c. nitrogen d. sodium e. sulfur

d. sodium

Atomic radius generally decreases as we move ____. a. down a group; the period position has no effect b. down a group and from left to right across a period c. up a group and from right to left across a period d. up a group and from left to right across a period e. down a group and from right to left across a period

d. up a group and from left to right across a period

Oxides of most nonmetals combine with base to form ____. a. an acid b. hydrogen gas c. water d. water and a salt e. a base

d. water and a salt

Oxides of the active metals combine with acid to form ____. a. metal hydroxides b. metal hydrides c. hydrogen gas d. water and a salt e. oxygen gas

d. water and a salt

In which orbital does an electron in a copper atom experience the greatest effective nuclear charge? a. 4p b. 4d c. 4s d. 3d e. 1s

e. 1s

Which alkaline earth metal will not react with liquid water or with steam? a. They all react with liquid water and with steam. b. Ca c. Mg d. Ba e. Be

e. Be

Of the following elements, ____ has the most negative electron affinity. a. Al b. Si c. P d. B e. Cl

e. Cl

Which element would be expected to have chemical and physical properties closest to those of rubidium? a. S b. Ca c. Cu d. Fe e. K

e. K

Which of the following generalizations cannot be made with regard to reactions of alkali metals? (The symbol M represents any one of the alkali metals.) a. 2M (s) + S (s) ® M2S (s) b. 2M (s) + 2H2O (l) ® 2MOH (aq) + H2 (g) c. 2M (s) + H2 (g) ® 2MH (s) d. 2M (s) + Cl2 (g) ® 2MCl (s) e. M (s) + O2 (g) ® MO2 (s)

e. M (s) + O2 (g) ® MO2 (s)

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? a. Mg > Na > P > Si > Ar b. Ar > Si > P > Na > Mg c. Ar > P > Si > Mg > Na d. Si > P > Ar > Na > Mg e. Na > Mg > Si > P > Ar

e. Na > Mg > Si > P > Ar

Which of the following is an isoelectronic series? a. F-, Cl-, Br-, I- b. S, Cl, Ar, K c. B5-, Si4-, As3-, Te2- d. Si2-, P2-, S2-, Cl2- e. O2-, F-, Ne, Na+

e. O2-, F-, Ne, Na+

Which of the following is an isoelectronic series? a. S, Cl, Ar, K b. B5-, Si4-, As3-, Te2- c. F-, Cl-, Br-, I- d. Si2-, P2-, S2-, Cl2- e. O2-, F-, Ne, Na+

e. O2-, F-, Ne, Na+

Of the elements below, ____ is the most metallic. a. Br b. Rn c. P d. As e. Sn

e. Sn

Element M reacts with chlorine to form a compound with the formula MCl2. Element M is more reactive than magnesium and has a smaller radius than barium. This element is ____. a. Na b. Ra c. K d. Be e. Sr

e. Sr

Element M reacts with oxygen to form an oxide with the formula MO. When MO is dissolved in water, the resulting solution is basic. Element M could be ____. a. selenium b. germanium c. bromine d. nitrogen e. strontium

e. strontium