Chemistry: Ch 7: Study Packet Flashcards

1) In which set of elements would all members be expected to have very similar chemical properties?

A) O, S, Se

B) N, O, F

C) Na, Mg, K

D) S, Se, Si

E) Ne, Na, Mg

2) In which set of elements would all members be expected to have very similar chemical properties?

A) P, Se, I

B) Cl, Br, Na

C) Si, As, Te

D) Ne, Na, Mg

E) Br, I, At

3) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ________ in Ar.

A) nuclear charge

B) paramagnetism

C) diamagnetism

D) Hund's rule

E) azimuthal quantum number

Screening of the nuclear charge by core electrons in atoms is ________.

A) less efficient than that by valence electrons

B) more efficient than that by valence electrons

C) essentially identical to that by valence electrons

D) responsible for a general decrease in atomic radius going down a group

E) both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group

5) The effective nuclear charge of an atom is primarily affected by ________.

A) inner electrons

B) outer electrons

C) nuclear charge

D) electron distribution

E) orbital radial probability

6) The atomic radius of main-group elements generally increases down a group because ________.

A) effective nuclear charge increases down a group

B) effective nuclear charge decreases down a group

C) effective nuclear charge zigzags down a group

D) the principal quantum number of the valence orbitals increases

E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases

7) Atomic radius generally increases as we move ________.

A) down a group and from right to left across a period

B) up a group and from left to right across a period

C) down a group and from left to right across a period

D) up a group and from right to left across a period

E) down a group; the period position has no effect

8) Atomic radius generally decreases as we move ________.

A) down a group and from right to left across a period

B) up a group and from left to right across a period

C) down a group and from left to right across a period

D) up a group and from right to left across a period

E) down a group; the period position has no effect

9) 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) Si > P > Ar > Na > Mg

D) Na > Mg > Si > P > Ar

E) Ar > P > Si > Mg > Na

10) Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr?

A) Ca > K > As > Ge > Kr

B) Kr > Ge > As > K > Ca

C) Ge > As > Kr > K > Ca

D) K > Ca > Ge > As > Kr

E) Kr > As > Ge > Ca > K

11) Of the compounds below, ________ has the smallest ionic separation.

A) KF

B) K2S

C) RbCl

D) SrBr2

E) RbF

12) Which of the following is an isoelectronic series?

A) B5-, Si4-, As3-, Te2-

B) F-, Cl-, Br-, I-

C) S, Cl, Ar, K

D) Si2-, P2-, S2-, Cl2-

E) O2-, F-, Ne, Na+

13) Which isoelectronic series is correctly arranged in order of increasing radius?

A) K+ < Ca2+ < Ar < Cl-

B) Cl- < Ar < K+ < Ca2+

C) Ca2+ < Ar < K+ < Cl-

D) Ca2+ < K+ < Ar < Cl-

E) Ca2+ < K+ < Cl- < Ar

14) Of the choices below, which gives the order for first ionization energies?

A) Cl > S > Al > Ar > Si

B) Ar > Cl > S > Si > Al

C) Al > Si > S > Cl > Ar

D) Cl > S > Al > Si > Ar

E) S > Si > Cl > Al > Ar

15) Of the choices below, which gives the order for first ionization energies?

A) Kr > Se > Br > Ga > Ge

B) Kr > Br > Se > Ge > Ga

C) Ga > Br > Ge > Kr > Se

D) Ga > Ge > Se > Br > Kr

E) Br > Se > Ga > Kr > Ge

16) ________ have the lowest first ionization energies of the groups listed.

A) Alkali metals

B) Transition elements

C) Halogens

D) Alkaline earth metals

E) Noble gases

17) Which of the following correctly represents the second ionization of aluminum?

A) Al+ (g) + e- → Al (g)

B) Al (g) → Al+ (g) + e-

C) Al- (g) + e- → Al2- (g)

D) Al+ (g) + e- → Al2+ (g)

E) Al+ (g) → Al2+ (g) + e-

18) Which of the following correctly represents the third ionization of aluminum?

A) Al2+ (g) + e- → Al+ (g)

B) Al (g) → Al+ (g) + e-

C) Al2- (g) + e- → Al3- (g)

D) Al2+ (g) + e- → Al3+ (g)

E) Al2+ (g) → Al3+ (g) + e-

19) Which of the following correctly represents the second ionization of phosphorus?

A) P+ (g) + e- → P2+ (g)

B) P (g) → P+ (g) + e-

C) P- (g) + e- → P2- (g)

D) P+ (g) → P2+ (g) + e-

E) P+ (g) + e- → P (g)

20) Which equation correctly represents the first ionization 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)

21) Which of the following correctly represents the second ionization of calcium?

A) Ca (g) → Ca+ (g) + e-

B) Ca+ (g) → Ca2+ (g) + e-

C) Ca- (g) + e- → Ca2- (g)

D) Ca+ (g) + e- → Ca2+ (g)

E) Ca+ (g) + e- → Ca (g)

22) Which of the following correctly represents the second ionization of copper?

A) Cu (g) → Cu+ (g) + e-

B) Cu+ (g) → Cu2+ (g) + e-

C) Cu- (g) + e- → Cu2- (g)

D) Cu+ (g) + e- → Cu2+ (g)

E) Cu+ (g) + e- → Cu (g)

23) Which ion below has the largest radius?

A) Cl-

B) K+

C) Br-

D) F-

E) Na+

24) Of the following species, ________ has the largest radius.

A) Rb+

B) Sr2+

C) Br-

D) Kr

E) Ar

Consider the following electron configurations to answer the questions that follow:

(i)1s2 2s2 2p6 3s1

(ii)1s2 2s2 2p6 3s2

(iii)1s2 2s2 2p6 3s2 3p1

(iv)1s2 2s2 2p6 3s2 3p4

(v)1s2 2s2 2p6 3s2 3p5

25) The electron configuration belonging to the atom with the highest second ionization energy is ________.

A) (i)

B) (ii)

C) (iii)

D) (iv)

E) (v)

Consider the following electron configurations to answer the questions that follow:

(i)1s2 2s2 2p6 3s1

(ii)1s2 2s2 2p6 3s2

(iii)1s2 2s2 2p6 3s2 3p1

(iv)1s2 2s2 2p6 3s2 3p4

(v)1s2 2s2 2p6 3s2 3p5

(26) The electron configuration that belongs to the atom with the lowest second ionization energy is ________.

A) (i)

B) (ii)

C) (iii)

D) (iv)

E) (v)

Consider the following electron configurations to answer the questions that follow:

(i)1s2 2s2 2p6 3s1

(ii)1s2 2s2 2p6 3s2

(iii)1s2 2s2 2p6 3s2 3p1

(iv)1s2 2s2 2p6 3s2 3p4

(v)1s2 2s2 2p6 3s2 3p5

27) The electron configuration of the atom with the most negative electron affinity is ________.

A) (i)

B) (ii)

C) (iii)

D) (iv)

E) (v)

Consider the following electron configurations to answer the questions that follow:

(i)1s2 2s2 2p6 3s1

(ii)1s2 2s2 2p6 3s2

(iii)1s2 2s2 2p6 3s2 3p1

(iv)1s2 2s2 2p6 3s2 3p4

(v)1s2 2s2 2p6 3s2 3p5

28) The electron configuration of the atom that is expected to have a positive electron affinity is ________.

A) (i)

B) (ii)

C) (iii)

D) (iv)

E) (v)

29) Of the following elements, ________ has the most negative electron affinity.

A) S

B) Cl

C) Se

D) Br

E) I

30) Of the following elements, ________ has the most negative electron affinity.

A) P

B) Al

C) Si

D) Cl

E) B

31) Of the following elements, ________ has the most negative electron affinity.

A) O

B) K

C) B

D) Na

E) S

32) Sodium is much more apt to exist as a cation than is chlorine. This is because ________.

A) chlorine is a gas and sodium is a solid

B) chlorine has a greater electron affinity than sodium does

C) chlorine is bigger than sodium

D) chlorine has a greater ionization energy than sodium does

E) chlorine is more metallic than sodium

33) Which equation correctly represents the electron affinity of calcium?

A) Ca (g) + e- → Ca- (g)

B) Ca (g) → Ca+ (g) + e-

C) Ca (g) → Ca- (g) + e-

D) Ca- (g) → Ca (g) + e-

E) Ca+ (g) + e- → Ca (g)

34) Which of the following correctly represents the electron affinity of bromine?

A) Br (g) → Br+ (g) + e-

B) Br (g) + e- → Br- (g)

C) Br2 (g) + e- → Br- (g)

D) Br2 (g) + 2e- → 2Br- (g)

E) Br+ (g) + e- → Br (g)

35) Which of the following correctly represents the electron affinity of phosphorus?

A) P (g) → P+ (g) + e-

B) P (g) + e- → P- (g)

C) P4 (g) + e- → P- (g)

D) P4 (g) + 4e- → 4P- (g)

E) P+ (g) + e- → P (g)

36) 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.

37) Of the elements below, ________ is the most metallic.

A) sodium

B) barium

C) magnesium

D) calcium

E) cesium

38) The list that correctly indicates the order of metallic character is ________.

A) B > N > C

B) F > Cl > S

C) Si > P > S

D) P > S > Se

E) Na > K > Rb

39) The list that correctly indicates the order of metallic character is ________.

A) Sr > Ca > Mg

B) F > Cl > Br

C) C > Ge > Si

D) Li > Na > K

E) O > Se > S

40) Of the elements below, ________ has the highest melting point.

A) Ca

B) K

C) Fe

D) Na

E) Ba

41) Of the following metals, ________ exhibits multiple oxidation states.

A) Al

B) Rb

C) Mg

D) Ni

E) Cs

42) Of the following oxides, ________ is the most acidic.

A) CaO

B) CO2

C) Al2O3

D) Li2O

E) Na2O

43) The acidity of carbonated water is due to the ________.

A) presence of sulfur

B) reaction of CO2 and H2O

C) addition of acid

D) nonmetal oxides

E) none of the above

44) The element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an electrical semiconductor is ________.

A) Sn

B) B

C) As

D) Si

E) Ge

45) Transition metals within a period differ mainly in the number of ________ electrons.

A) s

B) p

C) d

D) f

E) all of the above

46) Which one of the following compounds would produce an acidic solution when dissolved in water?

A) Na2O

B) CaO

C) MgO

D) CO2

E) SrO

47) Nonmetals can be ________ at room temperature.

A) solid, liquid, or gas

B) solid or liquid

C) solid only

D) liquid only

E) liquid or gas

48) Which of the following is not a characteristic of metals?

A) acidic oxides

B) low ionization energies

C) malleability

D) ductility

E) These are all characteristics of metals.

49) 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 gas at room temperature

B) a solid at room temperature

C) metallic

D) nonmetallic

E) a liquid at room temperature

50) Alkaline earth metals ________.

A) have the smallest atomic radius in a given period

B) form monoanions

C) form basic oxides

D) exist as triatomic molecules

E) form halides with the formula MX

51) Between which two elements is the difference in metallic character the greatest?

A) Rb and O

B) O and I

C) Rb and I

D) Li and O

E) Li and Rb

52) The oxide of which element below can react with hydrochloric acid?

A) sulfur

B) selenium

C) nitrogen

D) sodium

E) carbon

53) 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.

54) Which of the following traits characterizes the alkali metals?

A) very high melting point

B) existence as diatomic molecules

C) formation of dianions

D) the lowest first ionization energies in a period

E) the smallest atomic radius in a period

55) This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ________.

A) Na

B) Rb

C) Ca

D) Be

E) Fr