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Nine Weeks Test

Total questions: 25

Worksheet time: 13mins

Name
Class
Date
1.

The smallest bit of matter that is pure and can't be broken down into any other smaller substance by physical or chemical means.

a)

particle

b)

compound

c)

element

d)

Mixture

2.
Matter is classified into two main groups known as_______.
a)
solids and fluids
b)
pure substances and mixtures
c)
homogeneous and heterogeneous
d)
elements and compounds
3.
What is matter?
a)
Anything that has substance and takes up space.
b)
Stuff
c)
Has mass
d)
fluids and solids
4.
Pure oxygen (O) is an example of...
a)
an element
b)
a mixture
c)
a compound
5.
Combination of two or more substances that are not chemically combined.
a)
mixture
b)
solution
c)
solvent
d)
solute
6.
Kim puts an ice cube in a beaker and it melts. This is a good example of:
a)
a physical change.
b)
a chemical change.
c)
an experiment.
d)
an analysis.
7.

The order of elements in the periodic table is based on

a)

the number of protons in the nucleus.

b)

the electric charge of the nucleus.

c)

the number of neutrons in the nucleus.

d)

atomic mass.

8.

Atoms of elements that are in the same group have the same number of

a)

protons.

b)

neutrons.

c)

valence electrons.

d)

protons and neutrons.

9.

Which of the following elements is an alkali metal?

a)

calcium

b)

magnesium

c)

mercury

d)

sodium

10.

Metals tend to be

a)

gases.

b)

dull.

c)

brittle.

d)

good conductors.

11.

Which group is very stable due to the fact that they have a full outermost energy level?

a)

alkali metals

b)

halogens

c)

alkaline-earth metals

d)

noble gases

12.
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
13.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
14.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
15.
Which of the following will have a higher ionization energy than arsenic (As)?
a)
Gallium (Ga)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
16.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
17.

Which scientist's model is referred to as the Plum Pudding Model?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

18.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
19.
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
20.

How many dots would you put around carbon, a group 14 element?

a)

4

b)

6

c)

8

d)

18

21.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

22.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
23.
A molecule with a single covalent bond is....
a)
HCl
b)
SO
c)
CO
d)
SO2
24.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
25.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal

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