TRENDS IN THE PERIODIC TABLE
+1 +2
Number of Valence e- s
1
2
2
3
Electron dot diagram
X
X
X
X
Group
1
2
5
6
7
2
8
X
X
X
X
X
5
6
Transition elements (metals)
Metals
7

ATOMIC RADII
NON METALLIC PROPERTIES




Non-metals
ELECTRONEGATIVITY


4
13 14 15 16 17 18
IONIZATION ENERGY

-1
NON METAL REACTIVITY
METALLIC PROPERTIES
METAL REACTIVITY
ELECTRONEGATIVITY
IONIZATION ENERGY
ATOMIC RADII
4
-2
Halogens
3
-3
H
Alkaline earth metals
2
+3
Noble gases
1
Alkali metals
Period


Usual charge
REVIEW - PERIODIC TRENDS
1. -D-Which of the following properties is not characteristic of metals?
a) They are malleable.
b) They are good conductors of heat.
c) They are ductile.
d) They are dull in appearance.
2. -D-Which of the following elements is not a nonmetal?
a) fluorine
b) oxygen
c) nitrogen
d) antimony
3. -A-Which is the most reactive of all the elements?
a) fluorine
b) sodium
d) hydrogen
c) oxygen
4. -B-In Mendeleev's periodic table, the horizontal rows are called
a) groups
b) periods
c) families
d) columns
5. -D-Which group of the periodic table contains the least reactive elements?
a) alkali metals
b) halogens
c) actinides
d) noble gases
6. -C-Which of the following is the most metallic element?
a) oxygen
b) iron
c) potassium
d) neon
7. -B-Which of the following is the most non metallic element?
a) silicon
b) fluorine
c) nitrogen
d) helium
8. -A-Which of the following elements have atoms with four electrons in their outer energy levels?
a) carbon
b) oxygen
c) neon
d) boron
9. -B-An element that has an electron configuration of 1s2 2s22p6 3s23p5 is one of the
a) alkali metals
b) halogens
c) noble gases
d) transition metals
10. -D-An element that has an electron configuration of 1s2 2s22p6 3s23p6 4s2 3d5 is one of the
a) alkali metals
b) halogens
c) noble gases
d) transition metals
11. -A-Which of the following elements has the largest atomic radius?
a) beryllium
b) carbon
c) nitrogen
d) oxygen
12. -C-Which of the following elements has the smallest atomic radius?
a) sulfur
b) selenium
c) oxygen
d) tellurium
13. -C-Which of the following elements has the smallest first ionization energy?
a) strontium
b) calcium
c) barium
d) magnesium
14. -A-Which of the following elements has the largest first ionization energy?
a) bromine
b) potassium
c) arsenic
d) calcium
15. -A-Which of the following elements has the highest electron affinity?
a) chlorine
b) silicon
c) sodium
d) phosphorus
16. The following is a block of elements from the periodic table:
A
B
C
D
E
F
G
H
I
J
K
L
-I-a) which element has the largest atomic radius?
-D-b) which element has the smallest atomic radius?
17. Which atom in each of the following pairs has the higher ionization energy?
-Au-a) Cs or Au
-S-b) S or P
-Al-c) Mg or Al
-Rn-d) Rn or At
-Zn-e) Zn or Cu
-Sr-f) Rb or Sr
18. In each of the following pairs of elements, which has the higher ionization energy?
-O-a) O or S
-Se-b) Ge or Se
-Mg-c) Mg or Rb
-Xe-d) Xe or Cs
-Ne-e) Ne or Kr
-P-f) P or Si
19. Which element in the following sets loses an electron most readily; and why?
-Li-a) B, Li or F
-K-b) K, Li or Na
20. Which of the atoms has the lareest atomic radius?
-Na-a) Cl, Si or Na
-As-b) P, N or As
21. Which element is the most metallic?
-Ca-a) Mg, Ca or Be
-K-b) K, Br or Zn
22. Which group of elements is the most metallic?
Group 1 - Alkali metals
23. An element has the following ionization energies:
1st
7.6 eV
nd
2
l 5.0 eV
3rd
80.1 eV
Which group is the element a member of?
Group 2 – Alkaline Earth metals or any element that has only 2 valence electrons
24. Which group has the highest electronegativity?
Group 17 - Halogens
25. Which ion with a 3+ charge is isoelectronic with Ne?
Al3+
26. Write electron configurations for:
a) F
1s2 2s22p5 or [He] 2s22p5
b) O2- 1s2 2s22p6 or [He] 2s22p6
c) Cr
1s2 2s22p6 3s23p6 4s2 3d4 or
[Ar] 4s2 3d4
d) Pb
1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p2 or [Xe] 6s2 4f14 5d10 6p2
27. Complete the chart below:
Symbol
Ion Symbol
# p+
#e-
# n0
Al
[ Al 3+ ]
13
10
14
Cr
[ Cr 3+ ]
24
21
28
Br
  1- 

  Br



35
36
45
O
  2- 

  O

   
8
10
8
Fe
[ Fe 3+ ]
26
23
30
REVIEW - BONDING
1. -B-Ionic bonds are usually formed between two elements with the following combination of properties:
a) low ionization energy and low electronegativity.
b) low ionization energy and high electronegativity.
c) high ionization energy and low electronegativity.
d) high ionization energy and high electronegativity.
2. -C-An ionic bond is usually formed between
a) 2 nonmetals
b) 2 metals
c) a metal & a nonmetal
d) a metalloid & a nonmetal
3. -C-What is the correct formula for the ionic compound formed when Mg reacts with F?
a) MgF
b) Mg2F
c) MgF2
d) Mg2F3
4. -A-What is the formula of the ionic compound formed when element X (three valence electrons) reacts with
element Y (six valence electrons)?
a) X2Y3
b) XY
c) X2Y
d) X3Y2
5. -C-Which of the following is a property of ionic compounds?
a) Their solids conduct electricity.
b) They are usually gases or liquids at room temperature.
c) They have high melting points.
d) They are soft and waxy.
6. -D-Which of the following is isoelectronic with a noble gas?
a) [ F2-]
b) [ S-]
c) [ Al 2+]
d) [ Ca 2+ ]
7. -A-Which of the following has pure covalent bonding?
a) N2
b) HBr
c) MgF2
d) CH4
8. -A-Which of the following is a property of covalent compounds?
a) They have low boiling points.
b) They are hard and brittle.
c) Their molten state conducts electricity.
d) They have high melting points.
9. -B-Which of the following has polar covalent bonding?
a) F2
b) H2O
c) KC1
d) O2
10. -C-Element X has an electronegativity of 3.0 and element Y has an electronegativity of 1.0. The most probable type
of bond between X and Y is:
a) pure covalent
b) polar covalent
c) ionic
d) unpredictable
11. -B-Which of the following contains double bonding?
a) NH2CI
b) CS2
d) H2Te
12. -B-Which of the following contains triple bonding?
a) NBr3
b) C2Br2
c) C2C12
c) CO2
d) C2C14
13. Indicate which element(s) is slightly positive (δ+) and which element(s) is slightly negative (δ-) in the
following compounds:
a) Cl — F
b) Se = C = Se
c) H — C ≡ N
—
—
—
δ+ δδ+ δ- δ+
δ+ — δ+ — δ14. -A-Which bond is most polar?
a) O — H
b) C — H
c) C — C1
15. Draw the Lewis structures for the following compounds or ions, (some are ionic and some are covalent and some
are both). The brackets after an element indicates the number of that element if there is more than 1 compound
with that combination of elements. eg CO or CO2.
a) potassium & oxygen
+
-
3+
2-
O
K
b) boron and bromine
Br
B
2
3
c) calcium & oxygen
2+
Ca
d) lithium & chlorine
2-
O
e) magnesium & phosphorus
2+
+
2S
2
2
g) lithium & sulfur
h) iron (1) & bromine (3)
2-
S
Li
+
Cs
P
3
Cl
f) cesium & sulfur
3-
Mg
-
+
Li
-
3+
Br
Fe
3
2
i) nitrogen (1) & phosphorus (1)
N
P
Cl C C Cl
k) nitrogen (2) & oxygen (1)
N
j) carbon (2) & chlorine (2)
N O
m) carbon (1) & oxygen (2)
1) oxygen (2) and hydrogen (2)
H O O H
n) carbon (1) & oxygen (1)
C
O C O
o) CHCl3
O
p) NH3
H
Cl
C
Cl
H N H
H
Cl
q) HOCl
H O Cl
r) H2S
H S H
t) [ SO4 2- ]
s) Na2CO3
+
2-
O
Na
O
2
C
O
2-
O
O
S
O
O
v) [ NO3 1- ]
u) N2H4
H
H N
H
1-
O
N H
O
w) HCN
N
O
x) H2SO4
H C
O
N
H
O
S
O H
O
y) Ca3N2
z) SrBr2
3-
2+
N
Ca
3
2
2+
Sr
Br
2