WorksheetsComprehensive Chemistry Review Game
Total questions: 63
Worksheet time: 32mins
Unit Conversions 1. 1 kilometer = how many meters?
10
100
1,000
10,000
250 milliliters equals how many liters?
0.025 L
0.25 L
2.5 L
25 L
If an object has a mass of 500 grams and a volume of 250 mL, what is its density?
0.5 g/mL
2.0 g/mL
5.0 g/mL
0.25 g/mL
Which subatomic particle has a positive charge?
Proton
Neutron
Electron
Positron
Which particle has no charge?
Proton
Neutron
Electron
Ion
Most of an atom’s mass is located in the:
Nucleus
Electron cloud
Outer shell
Proton ring
The atomic number of an element tells you the number of:
Protons
Neutrons
Electrons in all shells
Valence electrons
What is the mass number of an atom with 10 protons and 12 neutrons?
10
22
12
2
An atom with 8 protons and 10 electrons has what kind of charge?
Neutral
+10
–2
+2
Isotopes of the same element differ in the number of:
Protons
Neutrons
Electrons
Valence electrons
A sodium atom becomes a Na⁺ ion by:
Losing one electron
Gaining one electron
Losing one proton
Gaining one neutron
Chlorine has isotopes with masses of 35 and 37. What is true?
They have the same number of protons but different neutrons
They have different numbers of protons
They are different elements
They have the same number of neutrons
How many electrons can the first energy level hold?
2
4
6
8
Which element has 3 valence electrons?
Oxygen
Nitrogen
Aluminum
Chlorine
In a Bohr model of carbon, how many electrons are in the outermost shell?
2
4
6
8
Elements in the same group (column) have:
The same number of neutrons
The same number of valence electrons
The same number of energy levels
The same mass number
Which of the following is a nonmetal?
Sodium (Na)
Oxygen (O)
Magnesium (Mg)
Iron (Fe)
Which region of the periodic table contains metalloids?
The staircase region between metals and nonmetals
On the far left
On the far right
Bottom two rows
Who proposed that atoms are indivisible solid spheres?
John Dalton
J.J. Thomson
Rutherford
Bohr
Who discovered the electron using the cathode ray tube?
Dalton
J.J. Thomson
Rutherford
Chadwick
Rutherford’s gold foil experiment showed that:
Electrons orbit randomly
Atoms have a dense, positively charged nucleus
Electrons are in fixed orbits
Neutrons exist in atoms
Bohr proposed that:
Electrons move in fixed energy levels
Atoms are solid spheres
Atoms are mostly empty space
Electrons have no mass
Which of these is the smallest particle of an element that retains its properties?
Atom
Molecule
Compound
Electron
Which element has the same number of protons and electrons as oxygen but a different number of neutrons?
An isotope of oxygen
Fluorine
Carbon
Neon
What happens to the number of energy levels as you move down a group in the periodic table?
Increases
Decreases
1 kilometer = how many meters?
10
100
1,000
10,000
1 gram = how many milligrams?
10
100
1,000
10,000
250 milliliters equals how many liters?
0.025 L
0.25 L
2.5 L
25 L
If an object has a mass of 500 g and a volume of 250 mL, what is its density?
0.5 g/mL
2.0 g/mL
5.0 g/mL
0.25 g/mL
What is the formula for density?
Density = Mass ÷ Volume
Density = Volume + Mass
Density = Mass × Volume
Density = Volume – Mass
An object with a density less than water (1 g/mL) will:
Sink
Float
Dissolve
Evaporate
If you double the volume but keep the same mass, the density will:
Stay the same
Be cut in half
Double
Increase slightly
Which subatomic particle has a positive charge?
Proton
Neutron
Electron
Positron
Which particle has no charge?
Proton
Neutron
Electron
Ion
Which particle is found in the electron cloud?
Proton
Neutron
Electron
Positron
Most of an atom’s mass is located in the:
Nucleus
Electron cloud
Outer shell
Proton ring
The atomic number equals the number of:
Protons
Neutrons
Electrons in all shells
Valence electrons
The mass number equals:
Protons only
Protons + Neutrons
Neutrons + Electrons
Protons – Neutrons
Isotopes differ in their number of:
Protons
Neutrons
Electrons
Energy levels
An atom with 8 protons and 10 electrons has a charge of:
+2
–2
Neutral
+10
A sodium atom becomes Na⁺ by:
Losing one electron
Gaining one electron
Gaining a proton
Losing a neutron
Chlorine becomes Cl⁻ by:
Losing an electron
Gaining an electron
Gaining a proton
Losing a neutron
The atomic number of carbon is 6. How many electrons are in a neutral atom of carbon?
6
8
12
3
Isotopes of carbon are C-12 and C-14. What do they have in common?
Same number of protons
Same number of neutrons
Different elements
Different atomic numbers
How many electrons fit in the first energy level?
2
4
6
8
How many electrons fit in the second energy level?
4
8
12
16
The outermost electrons are called:
Valence electrons
Core electrons
Shell electrons
Stable electrons
How many valence electrons does oxygen have?
2
6
8
4
Which element has 1 valence electron?
Sodium (Na)
Oxygen (O)
Carbon (C)
Neon (Ne)
In a Bohr model of nitrogen, how many electrons are in the 2nd shell?
3
5
7
8
What makes noble gases stable?
Full outer electron shell
Large number of neutrons
Equal protons and neutrons
Heavy atomic mass
Elements in the same group have the same number of:
Valence electrons
Neutrons
Protons
Shells
Elements in the same period have the same number of:
Valence electrons
Energy levels
Neutrons
Protons
Which element is a metalloid?
Sodium
Silicon
Iron
Neon
Which element is a halogen?
Oxygen
Chlorine
Potassium
Calcium
Metals are generally found on which side of the periodic table?
Left
Right
Middle
Top
Which property is true for metals?
Good conductors of heat and electricity
Dull and brittle
Poor conductors
Usually gases
Which element is a noble gas?
Oxygen
Fluorine
Neon
Hydrogen
Which subatomic particle determines the element’s identity?
Proton
Electron
Neutron
Isotope
What is the smallest particle that still retains chemical properties of an element?
Atom
Molecule
Proton
Compound
Which part of the atom determines its chemical reactivity?
Protons
Neutrons
Valence electrons
Nucleus
The nucleus contains:
Protons and neutrons
Electrons and neutrons
Protons and electrons
Only protons
Which is an example of a physical property?
Density
Reactivity with acid
Flammability
Rusting
