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Physical Science Semester I Review

Total questions: 50

Worksheet time: 2hrs 32mins

Name
Class
Date
1.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
2.
What subatomic particle is electrically neutral (no charge)?
a)
Proton
b)
Ion
c)
Neutron
d)
Electron
3.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
4.
How many protons does this atom have?
a)
2.5
b)
6
c)
5
d)
10.811
5.
In order for me to find the number of neutrons, I must round the atomic mass and then do what?
a)
atomic number-atomic mass
b)
atomic number x atomic mass
c)
atomic mass + atomic number
d)
atomic mass - atomic number
6.

How many neutrons are in Magnesium?

a)

36

b)

12

c)

24

d)

6

7.

How many electrons are in Sulfur?

a)

32

b)

16

c)

48

d)

8

8.

Which would you do to change this Lithium to a new element?

a)

Add a neutron

b)

Add an electron

c)

Add a proton

d)

Add a proton and neutron\

9.

Which atom will have a +1 charge?

a)

3 protons

4 neutrons

3 electrons

b)

3 protons

4 neutrons

4 electrons

c)

3 protons

4 neutrons

2 electrons

d)

3 protons

3 neutrons

3 electrons

10.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
11.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

12.

Found orbiting outside the nucleus, this subatomic particle has a negative charge.

a)

Neutron

b)

Proton

c)

Electron

d)

Idontknowatron

13.
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
14.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
15.

The common charge on an atom in group 17 would be....

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

16.

Which of the following reasons explains why there is a decimal for most atomic masses?

a)

The mass of one atom can have a fraction.

b)

Since electrons are very small mass they only add a little bit, usually only a decimals worth.

c)

It is the average mass of all the potential isotopes of an atom.

d)

Neutrons have a mass of 1.1 meaning that fractions are common.

17.
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 neutrons
18.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
19.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
20.
Vertical columns of elements (families) on the periodic table with similar  properties
a)
groups
b)
periods
c)
quadrants
d)
rows
21.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
22.

The horizontal (side to side) rows in the Periodic Table are called

a)

groups

b)

families

c)

periods

d)

atomic numbers

23.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
24.

How many valence electrons does a carbon atom have?

a)

8

b)

4

c)

2

d)

6

25.

If an element is in group number 15 you know it has _____ valence electrons.

a)

1

b)

2

c)

5

d)

15

26.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
27.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
28.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
29.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
30.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
31.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
32.
Predict the bond that will form between Se and Cl
a)
Ionic
b)
Covalent
33.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
34.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
35.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
36.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
37.

Is melting butter for popcorn a chemical or physical change?

a)

chemical

b)

physical

38.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
rust
39.
A change where one or more new substances are created.
a)
Physical Change 
b)
Chemical Change 
40.

Is this an example of a physical or chemical change?

a)

physical

b)

chemical

41.

The Law of Conservation of Mass States

a)

Energy cannot be created nor destroyed, it can only change form.

b)

Mass cannot be created nor destroyed, it can only change form.

c)

Mass can be created or destroyed, it cannot change form.

42.

Is the following equation balanced?

Al + O2 ---> 2Al2O3

a)

YES

b)

NO

43.

Is the following equation balanced?

2C2H2 + 5O2 ---> 4CO2 + 2H2O

a)

YES

b)

NO

44.

Three types of nuclear radiation are _______ radiation, _________radiation, and _____________ radiation.

a)

alpha, beta, and gamma

b)

theta, beta, and kappa

c)

alpha, beta, positron

45.

After one ____________ of a radioactive element, half of the original radioactive material remains.

a)

half-life

b)

cycle

c)

decay

46.

In a(n) ___________, particles released from one nuclear reaction collide with other particles and cause more nuclear reactions.

a)

nuclear fission reaction

b)

nuclear fusion reaction

47.

In ___ _____reactions, small nuclei combine, producing a large nucleus and releasing large amounts of energy.

a)

nuclear fission

b)

nuclear fusion

48.

What is the final stage in the life cycle of a low-mass star?

a)

supernova

b)

neutron star

c)

white dwarf

d)

black hole

49.
When a star's gravitational pull is so strong that not even light can escape, it's called a what?
a)
Black hole
b)
Supernova
c)
White dwarf
d)
Nebula
50.
What stage fills in the blank. Nebula --> Main sequence --> red giant --> ______________ --> white dwarf --> black dwaft
a)
supergiant
b)
planetary nebula
c)
black hole
d)
supernova

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