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Chemistry- Final Spring 2022

Total questions: 50

Worksheet time: 1hrs 17mins

Name
Class
Date
1.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
2.
The number at the bottom of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
chemical symbol
d)
element name
3.
The number at the top of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
Chemical Symbol
d)
Element Name
4.
These are found on the Periodic Table.
a)
Compounds
b)
Elements
c)
Mixtures
5.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
6.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
7.
Which statement about the atomic nucleus is correct?
a)
The nucleus is made of protons and neutrons and has a negative charge
b)
The nucleus is made of protons and neutrons and has a positive charge
c)
The nucleus is made of electrons and has a positive charge
d)
The nucleus is made of electrons and has a negative charge
8.
Most of the mass in an atom is concentrated in the...
a)
electrons
b)
nucleus
c)
protons
d)
empty space
9.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
10.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
11.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

12.

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

13.

What is the rule that elements want to have 8 valence electrons?

a)

Octet rule

b)

Octopus rule

c)

Valence electrons rule

d)

Ion rule

14.

What advantage does an element have when it has a full valence level of 8 electrons?

a)

Greater mass

b)

having more electrons is like having more money

c)

to over power teh effect of the protons

d)

stability

15.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
16.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
17.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

18.
Which of these elements has 8 valence electrons?
a)
P
b)
Be
c)
O
d)
Ar
19.

Which one of these is considered a SOLUTE?

a)

Salt

b)

Water

c)

Salt Water

20.

From the diagram in the previous slide which is solvent?

a)

Salt

b)

Water

c)

Salt Water

21.

From the diagram in the previous slide which is solution?

a)

Salt

b)

Water

c)

Salt Water

22.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
23.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
24.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)?

M = molLM\ =\ \frac{mol}{L}  

(HINT: Convert g to mol with the molar mass of NaOH first)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

25.

Calculate the molarity of the following solution: 1.0 mole of KCl in 750 mL of solution.  (HINT:  1000 mL = 1 L)

M = molLM\ =\ \frac{mol}{L}  

a)

0.750 M

b)

99 M

c)

1.3 M

d)

2.0 M

26.

What is the molarity of a solution made by adding 1.565 moles of Pb(NO3 )2 to enough water to make 500. mL of soution?

a)

300. M

b)

31.3 M

c)

3.13 M

d)

1.56 M

27.

If you have 2.5 moles of glucose in 0.5 L of solution, what is the concentration of the solution?

M = molLM\ =\ \frac{mol}{L}  

a)

0.5 M

b)

1.25 M

c)

2.5 M

d)

5 M

28.

Carbon has an atomic mass of 12. What is the mass of one mole of carbon

a)

6 grams

b)

12 grams

c)

120 grams

d)

1200000000 grams

29.

Hydrogen has an atomic mass of 1. Oxygen has an atomic mass of 16. What is the molar mass of water (H2O)

a)

1 gram

b)

16 grams

c)

18 grams

d)

14 grams

30.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
31.

What is the formula for Boyle's Law?

a)

P1V1=P2V2

b)

P1V1/P2V2

c)

P1V2=P2V1

d)

P1/V1=P2/V2

32.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
33.
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
a)
12.9 L
b)
0.72 L
c)
7.2 L
d)
3.44 L
34.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
35.
Volume and temperature have a ______ proportionality.
a)
direct
b)
inverse
c)
linear
d)
exponential
36.
At constant pressure, what happens to temperature of a gas when the volume doubles?
a)
The temperature also doubles.
b)
The temperature decreases to half of its original volume.
c)
The temperature doesn't change.
d)
The temperature quadruples.
37.

An inflated balloon with a volume of 0.85 L at 303 K was placed inside a freezer where the temperature is at -10 degrees Celsius. What is the final volume of the balloon if the pressure remains constant?

(a)  

38.

When the temperature of the gas is doubled, the volume gets ______________.

a)

doubled

b)

tripled

c)

remains constant

d)

reduced in half.

39.
In an exothermic process the surrounding looses heat. 
a)
True
b)
False
40.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
41.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
42.
Refer the the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
43.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
44.

___________________ is the capacity to do work or supply heat.

a)

energy

b)

heat changes

c)

specific heat

d)

thermochemistry

45.

What is calorimetry?

a)

process of measuring kinetic and potential energy

b)

process of measuring heat flow of chemical reactions

c)

process of measuring pressure and temperature of a substance

46.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

47.

What area of study in chemistry is concerned with the heat transfers that occur during chemical reactions?

a)

stoichiometry

b)

thermochemistry

c)

inorganic chemistry

d)

physical chemistry

48.

The law of conservation of energy states that

a)

in any chemical or physical change, energy cannot be created or destroyed, only changed in form.

b)

heat changes occur during chemical and physical changes.

c)

energy is the capacity to do work or to supply heat

d)

there are two types of energy, kinetic and potential

49.

The specific heat of a substance varies with the mass of a sample. True or False?

a)

True

b)

False

50.
When thermal energy is added to a substance, the substance's particles move:
a)
More rapidly at an increased diestance from each other.
b)
More rapidly with less distance between each other.
c)
More slowly with a greater distance between each other.
d)
More slowly with a reduced distance between each other.

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