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Periodic Table BIG Review

Total questions: 88

Worksheet time: 2hrs 10mins

Name
Class
Date
1.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
2.
Why were there blank spaces left in Mendeleev's periodic table?                                              
a)
He didn't know what to put there.
b)
 Undiscovered elements not yet known.
c)
Multiple elements could have fit
d)
He forgot to add the elements in.
3.
Who arranged the periodic table by increasing atomic number?
a)
Mendeleev
b)
Rutherford
c)
Bohr
d)
Mosely
4.
Which property did Mendeleev use to order his periodic table?
a)
Shielding effect
b)
Eletronegitivity
c)
Atomic Weight
d)
Metallic Character
5.
Each row in the periodic table is called a 
a)
group or family
b)
period
c)
cluster
d)
unit
6.
Each column in the periodic table is called a 
a)
period
b)
group or family
c)
cluster
d)
unit
7.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
8.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
9.
Elements which are shiny and conduct electricity and heat are called
a)
metals
b)
nonmetals
c)
metalloids
d)
nonexistent
10.
The yellow atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
11.
The atoms along the stair step or zig-zag line are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
12.
Which of the 3 major groups contains the most elements?
a)
Metals
b)
Metalloids
c)
Nonmetals
13.
Which element is not in the Alkali metal family?
a)
Li
b)
H
c)
Fr
d)
Cs 
14.
In what section would Transition Metals be found?
a)
orange
b)
light blue
c)
blue
d)
white
15.
The metals of group 2 are called
a)
transition metals
b)
alkaline earth metals
c)
lanthanides
d)
alkali metals
16.
The blue section is called the
a)
inner transition elements
b)
transition elements
c)
transuranium elements
d)
nonmetals
17.
The highlighted group is the 
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
18.
Elements that are gases, brittle and poor conductors are classified as what kind of elements?
a)
Nonmetals
b)
Metals
c)
Metalloids
d)
Alkali Metals
19.
Elements in the same group or family are expected to have  ________
a)
Similar Chemical Properties
b)
Same number of Protons
c)
Same Atomic number
20.
Which group on the Periodic Table has 3 Valence electrons(electrons on last energy level)?
a)
Group 13
b)
Group 3
c)
Group 17
21.
Group 2 Alkaline Earth elements are 
a)
more reactive than the alkali metals
b)
less reactive than the alkali metals
c)
unreactive
22.

The highlighted section is the...

a)

Actinides

b)

Lanthanides

c)

Halogens

d)

Alkali

23.

The highlighted section is the...

a)

Actinides

b)

Lanthanides

c)

Transition Metals

d)

Halogens

24.
Elements in the same period have
a)
same number of energy levels
b)
same number of protons
c)
same number of valence electrons
d)
similar physical and chemical properties
25.
How many valence electrons does magnesium have?
a)
1
b)
2
c)
12
d)
24
26.
How many valence electrons do atoms in group 16 have?
a)
4
b)
5
c)
6
d)
7
27.
What group number has 1 valence electron for each atom?
a)
group 1
b)
group 2
c)
group 10
d)
group 12
28.
Which of the following is the most reactive group of non-metals? 
a)
Oxygen family (Group 16)
b)
Noble Gases
c)
Halogens (Group 17)
d)
Nitrogen family (Group 15)
29.
Which statement is true about the properties of metalloids?
a)
Metalloids tend to have very similar properties to metals
b)
Metalloids tend to have very similar properties to nonmetals
c)
Metalloids tend to have properties that are a mixture of those of metals and nonmetals
d)
The properties of metalloids are completely different from both metals and nonmetals
30.
How many valence electrons does chlorine (Cl) have?
a)
2
b)
5
c)
6
d)
7
31.
How many valence electrons does carbon (C) have?
a)
3
b)
4
c)
5
d)
6
32.
Which of these elements has 8 valence electrons?
a)
P
b)
Be
c)
O
d)
Ar
33.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
34.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
35.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
36.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
37.
This is a correct dot diagram for neon (Ne)
a)
true
b)
false
38.

This could be the dot diagram of

a)

Ne

b)

H

c)

C

d)

F

39.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
40.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
41.
This could be the dot diagram of
a)
Be
b)
B
c)
C
d)
Ne
42.
This could be the dot diagram of
a)
Al
b)
Si
c)
Na
d)
Mg
43.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
44.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
45.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
46.
How many electrons should Magnesium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
47.
How many electrons should Boron have around its Lewis dot model?
a)
1
b)
3
c)
5
d)
7
48.
How many electrons should Chlorine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
49.

Which of the following would be the Lewis Dot Diagram for an ION of Aluminum?

a)
b)
c)
d)
50.

Which of the could represent an ION of sulfur?

a)
b)
c)
d)
51.

Which diagram could be showing an ion of Potassium?

a)
b)
c)
d)
52.

Based on the diagram, what group would element X be found in?

a)

2

b)

13

c)

15

d)

18

53.

This diagram is showing an ion from an element found in which group on the periodic table?

a)

Group 1

b)

Group 8

c)

Group 17

d)

Group -1

54.

What properites do nonmetals have in common?

a)

Poor conductor of electricity

b)

Good conductor of thermal energy

c)

Soft and Malleable

d)

Shiny, lustrous surface

55.

Elments which are semiconductors are classified as

a)

metals

b)

nonmetals

c)

metalloids

56.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
57.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
58.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
59.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
60.
The distance between the nucleus of an atom and the outer edge of the electron cloud
a)
Atomic radius
b)
Ionic Radius
c)
Ionization Energy
d)
Electronegativity
61.
Valence electrons are: 
a)
Electrons in the highest energy level
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons that are excited
62.

In moving from left to right across a period on the periodic table, the nuclear attraction for the valence electrons of an atom...

a)

increases

b)

decreases

c)

stays the same

63.

In moving from top to bottom down a group on the periodic table, ________________ for the valence electrons of the atom.

a)

nuclear attraction increases

b)

nuclear attraction decreases

64.

The minimum energy required to remove an electron from an atom

a)

electronegativity

b)

electron affinity

c)

ionization energy

d)

reactivity

65.

The tendency of an atom to attract electrons in a chemical bond

a)
electronegativity
b)
ionization energy
c)
electron affinity
d)
reactivity
66.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
67.
Put the following elements in order of decreasing ionization energy:
O, Te, Po, S.
a)
O, S, Po, Te
b)
O, S, Te, Po
c)
O, Te, Po, S
d)
O, Po, Te, S
68.
Which of the following would require the most energy to remove an electron?
a)
Sodium
b)
Potassium
c)
Rubidium
d)
Cesium
69.
Which of the following elements has the GREATEST electronegativity?
a)
Cl
b)
As
c)
Zn
d)
Na
70.
As one proceeds from fluorine to iodine in the Halogen family, the electronegativity ____.
a)
Decreases and atomic radius increases
b)
Decreases and atomic radius decreases
c)
Increase and atomic radius increases
d)
Increases and atomic radius decreases
71.
Put the following in order of increasing ionization energy:Tellurium, Sulfur, Selenium
a)
Tellurium, Sulfur, Selenium
b)
Selenium, Sulfur, Tellurium
c)
Sulfur, Selenium, Tellurium
d)
Tellurium, Selenium, Sulfur
72.
Put these in order of increasing electronegativity:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
73.
Why is potassium more reactive than sodium?
a)
Potassium is not more reactive than sodium
b)
Potassium has a lower ionization energy than sodium
c)
Potassium has a higher ionization energy than sodium
74.
Which statement is true?
a)
Cl has a higher electronegativity than Ar because it is farther to the left
b)
Ar has a higher electronegativity than Cl because it is farther to the right
c)
Ar does not have an electronegativity value because it has 8 valence electrons
75.
Why is I more reactive than Te?
a)
I has a higher electronegativity
b)
Te has a higher electronegativity
c)
I is not more reactive than Te
76.

Which of these best explains the reasoning behind the trend that as you go across a period, size decreases?

a)

As you go across a period, more energy levels are added, which shrinks the atom.

b)

The added electrons in the nucleus give the atom a negative charge, which shrinks the atom.

c)

The added protons in the nucleus pull the electrons closer to them, which shrinks the atom.

d)

All of the above

77.

Values for the first ionisation energies (IE) for five successive elements in the Periodic Table are given below (the letters are not their actual symbols). Based on these values, which statement is correct?

a)

Element M is a metal

b)

The outermost electron in element K is in a higher energy level than that in element L

c)

Element N is a non-metal

d)

Element P has a lower first ionisation than element O

78.

Which element can have the following ionization energies: 100, 700, 900, 1000?

a)

K

b)

Mg

c)

O

d)

F

79.

Where is there a big jump of ionization energy increase for successive ionizations of the element Silicon(Si)?

a)

between 1 and 2

b)

between 6 and 7

c)

between 7 and 8

d)

between 4 and 5

80.

Where is there a big jump of ionization energy increase for successive ionizations of the element Iodine(I) and why?

a)

between 6 and 7 because Iodine has 7 valence electrons

b)

between 7 and 8 because Iodine has 7 valence electrons

c)

between 6 and 7 because Iodine has 6 valence electrons

d)

between 7 and 8 because Iodine has 8 valence electrons

81.

The first seven ionisation energies of element M are 786, 1577, 3229, 4356, 16080, 19790 and 23780 kJ mol-1. In the Periodic Table, element M is in group

a)

3

b)

2

c)

12

d)

14

82.

Two elements that have similar physical and chemical properties are most likely in the same...

a)

period

b)

row

c)

group

83.

Which element is located in period 4?

a)

Zirconium (Zr)

b)

Silicon (Si)

c)

Beryllium (Be)

d)

Iron (Fe)

84.

What is the physical property on the Y-axis on the graph?

a)

Atomic Radius

b)

Ionic Radius

c)

Ionization Energy

85.
What trend is represented by this graph?
a)
Electronegativity
b)
Atomic Radius
c)
Ionic Radius
86.
In which quadrant of the periodic table would elements with the smallest atomic radius be found? 
a)
I
b)
II
c)
III
d)
IV
87.

Which data point represents a noble gas?

A
B
C
D
88.
The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?
a)
The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
b)
The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
c)
The ionization energy increases gradually as you move right across a period because you are adding more protons.
d)
The ionization energy increases when the valence electrons are more attracted to the nucleus.

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