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Periodic Table Test Review 25-26

Total questions: 40

Worksheet time: 33mins

Name
Class
Date
1.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

2.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

3.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

4.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

5.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

6.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

7.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

8.

Elements that have the same number of energy levels are said to be in the same ______.

a)

group

b)

period

c)

family

d)

classification

9.
What Periodic Table family is represented by the Lewis dot diagram?
a)
Halogens
b)
Alkali Metals
c)
Transition Metals
d)
Noble Gases
10.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
11.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
12.

Highly reactive

a)

Alkali metal

b)

Noble gases

c)

Rare earth metals

d)

Neon

13.

Which of the following is an inert gas?

a)

Hydrogen

b)

Helium

c)

Oxygen

d)

Carbon dioxide

14.

Noble gases are inert because

a)

They are highly reactive

b)

They are unreactive

c)

They are noble

d)

They have 8 electrons in their outer most energy level

15.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
16.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
17.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
18.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
19.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

20.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
21.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
22.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
23.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
24.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
25.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
26.

The vertical (up and down) columns in the periodic table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

27.

The horizontal (side to side) rows in the periodic table are called

a)

groups

b)

families

c)

periods

d)

atomic numbers

28.

The scientist ____ is credited with the idea of arranging the elements in the periodic table according to their physical and chemical properties.

a)

Mendeleev

b)

Dobereiner

c)

Newlands

d)

Dalton

29.

Mendeleev predicted that the empty spaces in his periodic table represented ____.

a)

isotopes

b)

radioactive elements

c)

permanent gaps

d)

undiscovered elements

30.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
31.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
32.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
33.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
34.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
35.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

36.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

37.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

38.

Ionization energy is ....

a)

the energy required to add an electron to an atom

b)

the energy required to shield the outer electrons from the nucleus

c)

a measure of the ability of an atom to attract electrons

d)

how much energy it takes to remove an electron from an atom

39.

Which is larger:

P or P-3 ?

a)

P because it is the neutral atom.

b)

P-3 because it lost 3 electrons.

c)

P-3 because it gained 3 electrons.

d)

They are the same size since they are both P.

40.

A sodium atom (Na) loses an electron to form a sodium ion (Na+1). Which statement is correct in regards to describing the ionic radius.

a)

The sodium ion (Na+1) has a larger radius than the neutral sodium atom (Na).

b)

The sodium ion (Na+1) has a smaller radius than the neutral sodium atom (Na).

c)

The sodium ion (Na+1) and the neutral sodium atom (Na) are the same size because they are both sodium.

d)

The sodium ion (Na+1) has twice the radius of the neutral sodium atom (Na).

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