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NGSS Chem IS3T2: Structure, Elect. Config, Metals & Nonmetal

Total questions: 61

Worksheet time: 52mins

Name
Class
Date
1.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
2.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
3.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
4.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

5.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

6.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
7.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
8.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
9.

Two objects that are similarly charged will...

a)

attract.

b)

repel.

c)

not experience an electric force.

d)

implode.

10.

A negatively charged object and a positively charged object will...

a)

attract.

b)

repel.

c)

not experience an electric force.

d)

implode.

11.

An object becomes positively charged by...

a)

gaining negative charges.

b)

losing negative charges.

c)

gaining positive charges.

d)

losing positive charged.

12.

An object becomes negatively charged by...

a)

gaining negative charges.

b)

losing negative charges.

c)

gaining positive charges.

d)

losing positive charged.

13.

Which of the following is not a way that ions can form?

a)

gaining electrons

b)

gaining protons

c)

losing electrons

d)

All of the above are ways that ions can form.

14.

Oxygen has six valence electrons. When forming an ion, oxygen will

a)

lose six electrons and have a charge of +6.

b)

lose six electrons and have a charge of -6.

c)

gain two electrons and have a charge is +2.

d)

gain two electrons and have a charge of -2.

15.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

16.

Most elements are most stable when their outermost energy levels contain ________ electrons.

a)

2

b)

6

c)

8

d)

18

17.

Look at the Periodic table. Which of the following elements would you expect to form an ion that has the same charge as the oxide ion?

a)

calcium

b)

boron

c)

sulfur

d)

chlorine

18.

Which of the following groups on the Periodic Table will only form ions with positive charges?

a)

Group 2

b)

Group 15

c)

Group 17

d)

Group 18

19.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
20.

What is a charged atom known as?

a)

Electron

b)

Proton

c)

Ion

d)

Neutron

21.
What charge will a Beryllium ion have?
a)
+
b)
2+
c)
2-
d)
-
22.
What charge will a sulfide ion have?
a)
3+
b)
2+
c)
2-
d)
3-
23.
How many electrons are in a Li+ ion?
a)
1
b)
2
c)
3
d)
4
24.
Subatomic particle with a charge of 0
a)
neutron
b)
proton
c)
electron
d)
quark
25.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

26.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
27.

These are found in the nucleus and have a neutral charge.

a)

proton

b)

electron

c)

neutron

28.
These will determine what element an atom is. 
a)
number of neutrons
b)
number of electrons
c)
number of atoms 
d)
number of protons 
29.

The number 16 for the atomic element sulfur is the

a)

ionic number

b)

isotope

c)

atomic mass

d)

atomic number

30.

How many protons does sulfur have?

a)

32

b)

16

c)

48

d)

12

31.

How many electrons does sulfur have

a)

16

b)

32

c)

48

d)

12

32.

In an atom, the number of protons is equal to the number of ____________.

a)

energy levels

b)

neutrons

c)

neurons

d)

electrons

33.
What is the atomic mass of "F"
a)
9
b)
18
c)
17
d)
19
34.
An atom of the element with atomic number 6 always has _____.
a)
six protons in its nucleus
b)
an atomic mass of six
c)
more than six neutrons
d)
six electron clouds
35.
What are subatomic particles? 
a)
the nucleus 
b)
electron cloud
c)
positive charge
d)
electrons, protons, and neutrons
36.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
37.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
38.

How many electrons does an Iodine atom have?

a)

53

b)

126

c)

73

d)

179

39.
How many protons are in Beryllium?
a)
4
b)
9
c)
5
d)
2
40.
Subatomic particle with a charge of 0
a)
neutron
b)
proton
c)
electron
d)
quark
41.
a)
2
b)
8
c)
3
d)
13
42.
a)
12
b)
7
c)
8
d)
14
43.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
44.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

45.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

46.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
47.
How many valence electrons are found in atoms of group 14?
a)
4
b)
3
c)
14
d)
16
48.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
49.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons in the second shell
50.
How many valence electrons are in an atom of Ba?
a)
2
b)
8
c)
4
d)
1
51.

Which metal is more reactive than calcium?

a)

magnesium

b)

potassium

c)

silver

d)

aluminum

52.

Rank the following by decreasing reactivity:

I, Kr, Sb, Te

a)

I, Te, Sb, Kr

b)

Kr, I, Te, Sb

c)

Kr, Sb, Te, I

d)

Sb, Te, I, Kr

53.

The trend for reactivity for metals is that the reactivity _______ as you go across the period and it _________ as you move down a group.

a)

increases, increases

b)

decreases, decreases

c)

does not change, decreases

d)

decreases, increases

54.

The trend for reactivity for nonmetals is that as you move across from left the right reactivity __________(except for noble gases) and as you move down a group the reactivity _________

a)

increases, increases

b)

decreases, decreases

c)

decreases, increases

d)

increases, decreases

55.

Which of the following nonmetals are the most reactive?

a)

Ge

b)

Kr

c)

Se

d)

Br

56.

Which of the following nonmetals are the most reactive?

a)

Po

b)

S

c)

Se

d)

O

57.

What is the most reactive nonmetal?

a)

I

b)

F

c)

N

d)

At

58.

What is the most reactive metal?

a)

Li

b)

Be

c)

Fr

d)

H

59.

Metals that are the most reactive have the following characteristics

a)

small atomic radius, high ionization energy, high electronegativity

b)

large atomic radius, high ionization energy, low electronegativity

c)

large atomic radius, low ionization energy, low electronegativity

d)

small atomic radius, low ionization energy, low electronegativity

60.

The most reactive nonmetals have _____ valence electrons

a)

1

b)

2

c)

7

d)

8

61.

Metals are electron _______ because they tend to _______ electrons in order to become stable like the noble gases.

a)

takers, lose

b)

takers, gain

c)

givers, gain

d)

givers, lose

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