CHPT. 5 QUIZ

Arrange the following elements in order of increasing first ionization energy. Mg, Al, Si, P, S A. Al < Mg < Si < S < P B. Mg < Al < Si < P < S C. Al < Mg < Si < P < S D. Mg < Al < Si < S < P E. Al < Mg < P < Si < S

Al < Mg < Si < S < P

Which ion has the largest radius? A. F− B. Cl− C. Br− D. I− E. At−

At-

Which element has the highest first ionization energy? A. B B. Al C. Ga D. In E. Tl

B

Arrange the following elements in order of decreasing first ionization energy. Be, Ca, Cs, Mg, K A. Mg > Be > Ca > K > Cs B. Be > Mg > Ca > K > Cs C. Cs > K > Ca > Be > Mg D. Ca > Mg > Be > Cs > K E. Ca > Mg > Be > K > Cs

Be > Mg > Ca > K > Cs

Which of these elements has the greatest attraction for electrons in a covalent bond? A. Ge B. As C. Se D. Br E. Kr

Br

Which element has the highest electronegativity? A. C B. Si C. Ge D. Sn E. Pb

C

Which pair of elements below would be least likely to form an ionic bond between them? A. Na / S B. C / N C. Al / F D. Mg / Br E. Cs / O

C / N

Which equation below depicts the reaction from which the first ionization energy would be determined? A. Ca(g) → Ca+(g) + e− B. Ca(s) → Ca+(g) + e− C. Ca(s) + e− → Ca-(g) D. Ca(g) → Ca2+ + e− E. None of these

Ca(g) → Ca+(g) + e−

Arrange the following set of ions in order of increasing ionic radii. Ca2+, Cl−, K+, P3−, S2− A. Ca2+ < K+ < P3− < S2− < Cl− B. Ca2+ < K+ < Cl− < S2− < P3− C. K+ < Cl− < Ca2+ < S2− < P3− D. Cl− < S2− < P3− < Ca2+ < K+ E. P3− < S2− < Cl− < K+ < Ca2+

Ca2+ < K+ < Cl− < S2− < P3−

Arrange the following elements in order of increasing atomic radii. K, Na, Mg, Cs, Cl A. Na < Mg < Cl < K < Cs B. Cl < Mg < Na < K < Cs C. Cs < K < Cl < Mg < Na D. Cl < Mg < Cs < K < Na E. Cl < Mg < Na < Cs < K

Cl < Mg < Na < K < Cs

Arrange the following elements in order of increasing values of electron affinity, i.e., from most negative to least negative. (Note: None of these elements is an exception to the general trends of electron affinities.) Cl, Se, S, Cs, Rb, Te A. Cl < S < Se < Rb < Te < Cs B. Cl > Te > Se > S > Rb > Cs C. Cl > Se > S > Te > Rb > Cs D. Cl < S < Se < Te < Cs < Rb E. Cl < S < Se < Te < Rb < Cs

Cl < S < Se < Te < Rb < Cs

Which element has the lowest electronegativity? A. H B. Li C. Na D. K E. Cs

Cs

Which ion has the smallest radius? A. F− B. Cl− C. Br− D. I− E. At−

F-

Arrange the following elements in order of increasing atomic radii. Sr, Rb, Sb, I, In A. Rb < Sr < In < Sb < I B. I < Sb < In < Rb < Sr C. In < Sb < I < Sr < Rb D. Sb < I < In < Sr < Rb E. I < Sb < In < Sr < Rb

I < Sb < In < Sr < Rb

Which of these comparisons according to radius is (are) correct? I. Na+ > Mg2+ II. In3+ > Sr2+ III. Cl− > K+ IV. Cl > K

I. and III.

Which element has the lowest electronegativity? A. K B. Ca C. Ga D. Ge E. As

K

Which comparison of electronegativities is not correct? A. Br > Se B. K > Mg C. O > S D. N > Be E. I > Ba

K > Mg

Which element has the highest electronegativity? A. N B. Si C. As D. P E. C

N

Which ion has the largest radius? A. Li+ B. Na+ C. Be2+ D. Mg2+ E. Al3+

Na+

Which one of the following pairs contains isoelectronic species? A. Na / Na+ B. S / Se C. S2− / Se2− D. F2 / Cl2 E. Na+ / O2−

Na+ / O2−

Arrange the following elements in order of decreasing electronegativities. Al, Cs, Mg, Na, P A. P > Al > Mg > Na > Cs B. Cs > Na > Mg > Al > P C. Al > Mg > Na > Cs > P D. P > Al > Mg > Cs > Na E. P > Cs > Na > Mg > Al

P > Al > Mg > Na > Cs

Arrange the following elements in order of decreasing atomic radii. Pb, P, Cl, F, Si A. Cl > F > Pb > Si > P B. Pb > Si > P > F > Cl C. Pb > Si > P > Cl > F D. Pb > Cl > P > Si > F E. Pb > Cl > P > Si > F

Pb > Si > P > Cl > F

Which ion has the largest radius? A. O2− B. S2− C. Se2− D. Te2− E. Po2−

Po2-

Arrange the following elements in order of increasing electronegativities. Mg, Ra, P, Cl, Al A. Mg < Ra < P < Al < Cl B. Ra < Mg < Al < P < Cl C. Mg < Ra < P < Cl D. Al < P < Cl < Mg < Ra E. Al < P < Cl < Ra < Mg

Ra < Mg < Al < P < Cl

Which element has the lowest electronegativity? A. Mg B. Na C. Rb D. Y E. Sc

Rb

Which of the following pairs of elements would be expected to form an ionic compound? A. S / F B. H / C C. Rb / Cl D. As / Br E. C / I

Rb / Cl

Arrange the following set of ions in order of decreasing ionic radii. Al3+, Ga3+, Ca2+, Rb+, K+ A. Rb+ > Ga3+ > Ca2+ > K+ > Al3+ B. Rb+ > K+ > Ca2+ > Al3+ > Ga3+ C. Ga3+ > Al3+ > Ca2+ > Rb+ > K+ D. Rb+ > Ca2+ > K+ > Ga3+ > Al3+ E. Rb+ > K+ > Ca2+ > Ga3+ > Al3+

Rb+ > K+ > Ca2+ > Ga3+ > Al3+

Which of the following elements has the most negative electron affinity? A. Si B. P C. S D. Se E. Te

S

Which of the lists of increasing ionic radii is not correct? A. Cl− < Br− < I− B. Al3+ < Mg2+ < Na+ C. Ca2+ < Sr2+ < Ba2+ D. S2− < Cl− < K+ E. Na+ < O2− < N3−

S2- < Cl < K+

Which ion or atom has the largest radius? A. S B. S2− C. Se D. Se2− E. Br

Se2−

Which ion has the smallest radius? A. As3− B. Se2− C. Br− D. Rb+ E. Sr2+

Sr2+

Which ion has the smallest radius? A. K+ B. Cs+ C. Sr2+ D. Ba2+ E. Tl3+

Tl3+

The amount of energy absorbed in the process in which an electron is added to a neutral gaseous atom is defined as ____. A. shielding effect B. electronegativity C. electron affinity D. first ionization energy E. standard reduction potential

electron affinity

A property that measures the ability of an atom to attract electrons in a chemical bond is A. binding energy. B. mass defect. C. electron affinity. D. ionization energy. E. electronegativity.

electronegativity

The minimum energy required to remove the most loosely held electron is A. first ionization energy. B. electron affinity C. potential energy D. kinetic energy E. electronegativity.

first ionization energy.

As we move across the periodic table from left to right, atoms become smaller due to A. increasing effective nuclear charge. B. the p orbitals being filled. C. electron-electron repulsions. D. shell size increases. E. none of these.

increasing effective nuclear charge.

What would be the outer electron configuration of alkaline earth metals? A. ns2np2 B. np2 C. ns0np2 D. nd2 E. ns2

ns2

What would be the outer electron configuration of group VIA (O, S, Se, . . .)? A. ns2np6 B. ns2np2 C. ns2np4 D. np6 E. ns0np6

ns2 np4

The general electron configuration for the element group that would have the largest negative value for the electron affinity for its atoms is ____? A. ns2np6 B. ns2np4 C. ns1 D. ns2np5 E. ns2np3

ns2 np5

The first ionization energy of sulfur is less than that of phosphorus. A reasonable explanation for this fact involves A. the stability of the half-filled subshell in atomic sulfur. B. pairing of two electrons in one 3p orbital in sulfur atoms. C. the smaller size of sulfur atoms relative to phosphorus atoms. D. the ease with which phosphorus attains a noble gas electronic configuration. E. the higher electronegativity of sulfur relative to phosphorus.

pairing of two electrons in 3p orbital in sulfur atoms.

Simple positively charged ions are always ____ than the neutral atoms from which they are formed. A. smaller B. larger C. isoelectronic D. the same size E. more anionic

smaller

Which electrons have the greatest influence on the properties of elements? A. those electrons in s orbitals B. those electrons in d orbitals C. core electrons D. the outermost electrons E. none of these

the outermost electrons

Accordingly to the periodic law the properties of elements repeat at regular intervals when the elements are arranged in order of A. their increasing atomic mass. B. their increasing atomic size. C. their increasing number of neutrons in the nucleus. D. their increasing number of isotopes. E. their increasing number of protons in the nucleus.

their increasing number of protons in the nucleus.