Ch. 5 Chemical Periodicity
What would be the outer electron configuration of group IIIB (Sc, Y, La . . .)?
(n − 1)d1ns2
their increasing number of protons in the nucleus.
Accordingly to the periodic law the properties of elements repeat at regular intervals when the elements are arranged in order of
Which element has the largest atomic radius?
Al
P > Al > Mg > Na > Cs
Arrange the following elements in order of decreasing electronegativities. Al, Cs, Mg, Na, P
Be > Mg > Ca > K > Cs
Arrange the following elements in order of decreasing first ionization energy. Be, Ca, Cs, Mg, K
Ra < Mg < Al < P < Cl
Arrange the following elements in order of increasing electronegativities. Mg, Ra, P, Cl, Al
Al < Mg < Si < S < P
Arrange the following elements in order of increasing first ionization energy. Mg, Al, Si, P, S
Cl < S < Se < Te < Rb < 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.)
Rb+ > K+ > Ca2+ > Ga3+ > Al3+
Arrange the following set of ions in order of decreasing ionic radii. Al3+, Ga3+, Ca2+, Rb+, K+
Arrange the following elements in order of decreasing first ionization energy. Rb, In, Sn, Sb, As
As > Sb > Sn > In > Rb
increasing effective nuclear charge.
As we move across the periodic table from left to right, atoms become smaller due to
Which ion has the largest radius?
At−
Which element has the highest first ionization energy?
B
Which element has the highest electronegativity?
C
Which equation below depicts the reaction from which the first ionization energy would be determined?
Ca(g) → Ca+(g) + e−
Arrange the following set of ions in order of increasing ionic radii. Ca2+, Cl−, K+, P3−, S2−
Ca2+ < K+ < Cl− < S2− < P3−
Which element has the smallest radius?
Cl
Arrange the following elements in order of increasing atomic radii. K, Na, Mg, Cs, Cl
Cl < Mg < Na < K < Cs
Which of the following is not a representative element?
Co
Which element has the lowest electronegativity?
Cs
Which element has the lowest first ionization energy?
Cs
Arrange the following elements in order of decreasing first ionization energy. F, Be, O, N, C
F > N > O > C > Be
Which ion has the smallest radius?
F−
Arrange the following elements in order of increasing atomic radii. Sr, Rb, Sb, I, In
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?
K
Which element has the highest electronegativity
N
Which ion has the largest radius?
Na+
Which ion has the smallest radius?
O2-
Which of the following ions is not isoelectronic with a noble gas
P2-
Arrange the following elements in order of decreasing atomic radii. Pb, P, Cl, F, Si
Pb > Si > P > Cl > F
Which element has the lowest electronegativity?
Rb
Which of the following elements has the most negative electron affinity?
S
Which ion or atom has the largest radius?
Se2−
Which element has the largest atomic radius?
Sn
Which element has the largest atomic radius?
Sr
Which ion has the smallest radius?
Sr2+
Which has the smallest radius?
Te
electron affinity
The amount of energy absorbed in the process in which an electron is added to a neutral gaseous atom is defined as ____.
pairing of two electrons in one 3p orbital in sulfur atoms.
The first ionization energy of sulfur is less than that of phosphorus. A reasonable explanation for this fact involves
ns2np5
The general electron configuration for the element group that would have the largest negative value for the electron affinity for its atoms is ____?
first ionization energy
The minimum energy required to remove the most loosely held electron is
Which ion has the smallest radius?
Tl3+
ns2np4
What would be the outer electron configuration of group VIA (O, S, Se, . . .)?
K > Mg
Which comparison of electronegativities is not correct?
Ar
Which element has the highest first ionization energy?
P
Which element has the smallest radius?
Po2−
Which ion has the largest radius?
Rb / Cl
Which of the following pairs of elements would be expected to form an ionic compound?
S2− < Cl− < K+
Which of the lists of increasing ionic radii is not correct?
Br
Which of these elements has the greatest attraction for electrons in a covalent bond?
Na+ / O2−
Which one of the following pairs contains isoelectronic species?
C / N
Which pair of elements below would be least likely to form an ionic bond between them?
Cr
____ is a d-transition metal.
A property that measures the ability of an atom to attract electrons in a chemical bond is
electronegativity
Choose the term that best describes all members of this series of elements: Xe, Rn, He, Ne, Kr
noble gases
Of the following, which periodic group(s) do not match their designation?
noble gases / VIIIB
What would be the outer electron configuration of alkaline earth metals?
ns2
Simple positively charged ions are always ____ than the neutral atoms from which they are formed.
smaller
Which electrons have the greatest influence on the properties of elements?
the outermost electrons
