Honors Chemistry
Name ___________________________
Period _______
Date _____________
Ch. 7 – Elements’ Periodic Trends WS 1
1) Mark the following elements as: transition metal (TM), Alkali Metal (AM), Alkaline Earth Metal
(AEM), Noble Gas (NG), Halogen (H), Metalloid (Moid) or inner transition element (IT).
Be ______
K ______
Cr ______
Kr ______
Si ______
Am ______
F ________
2) According to the periodic law, when the elements are arranged in the order of their ________________,
their properties show periodicity.
3) Elements that conduct heat and electricity well are classified as ____________________.
4) Elements that do not conduct heat and electricity well are gases and brittle solids. These elements are
classified as ________________ and _________________.
5) How many electrons are in the valence shell of
Na _____
Ca ____
F ____
Cl ____
O _____
Al _____
C ______
6) Energy required to remove an electron from an atom: __________________________energy.
7) Which element in each pair has the greater ionization energy?
a) He or O,
b) Na or F,
c) Ca or Br,
d) K or S.
8) Which element in each pair has the larger atoms?
a) Li or K
b) F or Br,
c) Na or S,
d) B or In.
9) In which group would elements with the following electron configurations be found?
a) 2-8-1: __________
b) 2-8-4: ___________
c) 2-8-8-2: ___________
10) Which group of elements has the highest ionization energies? _______________
11) Which group of elements has the lowest ionization energies? _______________
12) Which group of elements tends to have high electron affinities? _____________
13) Which group of elements has the largest atomic radius? ______________
14) a) Define: Effective Nuclear Charge (Zeff):
b) What is the magnitude of Zeff for the following elements:
Na
Zeff =
Mg
Zeff =
Al
Zeff =
P
Zeff =
Cl
Zeff =
1
15) Circle the element that correlates with the statement:
(a) highest ionization energy
S, Se, Te
(b) smallest radius
F-, Cl-, Br-
(c) lowest electron affinity
Ba, Sr, Cs
(d) largest ionization energy
O, S, F
(e) largest ionic radius
Mg2+, Ca2+, Ba2+
(f)
S
largest radius
2-
Cl- , Cl
(g) highest ionization energy
B, C, N
(h) highest electron affinity
P, S, Cl
(i) smallest atom
Sn, Te, Xe
(j) lowest ionization energy
Rb, Na, Mg
16) Identify the atom or ion with the larger radius in each of the following pairs:
(a) Cl or S
(b) Cl- or S2-
(c) Na or Mg
(d) Mg2+ or Al3+
17) Which atom or ion has the smaller radius:
(a) Li+ or Na+
(b) Cl or Cl-
(c) Al or Al3+
(d) N3- or F-
18) Predict which atom of each pair has the greater first ionization energy :
(a) Na or Mg
(b) C or N
(c) P or Sb
19) Predict which atom of each pair has the greater first ionization energy :
(a) Ba or Ca
(b) Cl or I
(c) Ar or Xe
20) Arrange the elements S, As, F, Zr and Cd in order of increasing electronegativity (lowest to highest):
21) In each set, select the element that has the greatest electronegativity:
(a) Cl, P, or S
(b) F, O, or S
(c) Sr, In or Ge
22) In each of the following pairs, identify the element that tends to acquire electrons from the other when
forming a bond:
(a) O and Ca
(b) Mg and F
(c) Br and Fe
23) In each of the following pairs, identify the element that tends to acquire electrons from the other when
forming a bond:
(a) S and Ni
(b) O and Al
(c) Cl and Ba
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