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Worksheets

TEKS Review

Total questions: 60

Worksheet time: 1hrs 23mins

Name
Class
Date
1.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
2.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

3.

When the temperature increases, it is an _______ reaction.

a)

Exothermic

b)

c)

Endothermic

d)

4.
In heat transfer, heat always flows from the _______________ substance to the _______________ substance.
a)
Hotter to colder
b)
Colder to hotter
c)
Hotter to hotter
d)
Colder to colder
5.

Two objects have different temperatures. Object A has a temperature of 42 degrees and Object B is 37 degrees. Which direction should the energy transfer between Objects A and B?

a)

From Object A to Object B

b)

From Object B to Object A

c)

Energy will not transfer

d)

Energy will transfer both directions

6.

What occurs when thermal equilibrium is reached within a system?

a)

The system cools down rapidly.

b)

Heat transfer stops completely.

c)

All substances within the system have the same temperature.

d)

Thermal energy flows in the opposite direction.

7.

An atom has 7 protons, 8 neutrons, and 8 electrons. What is the atomic number

a)

7

b)

8

c)

15

d)

23

8.

An atom has 7 protons, 8 neutrons, and 8 electrons. What is the mass number?

a)

7

b)

8

c)

15

d)

23

9.

An atom has 7 protons, 8 neutrons, and 8 electrons. What is the name of the element?

a)

Carbon

b)

Oxygen

c)

Nitrogen

d)

Phosphorus

10.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

11.

Ions of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

12.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

13.
Ernst Rutherford discovered which part of the atom through the use of gold foil?
a)

nucleus

b)

Neutron

c)

Electron

d)

Orbitals

14.

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

a)

Atom is mostly empty space

b)

The nucleus is positively charged

c)

The atom has a small dense nucleus

d)

All answers are correct

15.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
16.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
17.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
18.
What waves have the lowest energy? 
a)
Gamma rays
b)
Visible light waves
c)
Radio waves
d)
X rays
19.

Which color has the longest wavelength?

a)

Yellow

b)

Red

c)

Green

d)

Purple

20.

What is the correct order of the visible light spectrum starting with the longer wavelength?

a)

Red, yellow, orange, blue, violet, indigo

b)

Violet, indigo, blue, green, yellow, orange, red

c)

Green, yellow, blue, indigo, red, orange

d)

Red, orange, yellow, green, blue, indigo, violet

21.

The diagram below shows the electromagnetic spectrum. Which letters represent radio and gamma waves?

a)

A F

b)

F C

c)

A G

d)

C G

22.

Which of the following types of electromagnetic waves have the shortest wavelength?

a)

infrared waves

b)

x-rays

c)

radio waves

d)

ultraviolet waves

23.
This is a correct dot diagram for nitrogen (N)
a)
true
b)
false
24.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
25.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
26.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
27.
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
28.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
29.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

30.

Elements in the same group have the same

a)

Properties

b)

Number of electrons

c)

Number of protons

d)

Nucleus

31.
Group 18 elements are known as the _____ _____ and have full valence shells.
a)
royal gases.
b)
supreme solids.
c)
noble gases.
d)
legit liquids.
32.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
33.
Name group 1 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens
34.
Name group 17 on the periodic table.
a)
transition metals
b)
metalloids
c)
halogens
d)
alkali metals
35.

This group of highly reactive non-metals on the periodic table has elements in solid, liquid, and gas states of matter

a)

Alkali Metals

b)

Actinides and Lanthanides

c)

Halogens

d)

Noble Gasses

36.

The most reactive metals on the periodic table are the

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

37.

Ionic Bonding is the _________ of electron/s between atoms.

a)

sharing

b)

transfer

c)

loose

d)

gain

38.

This refers to the tendency of atoms to prefer to have eight electrons in the valence shell

a)

Octet rule

b)

Valence electron

c)

Electronegativity

d)

Lewis symbol

39.

A bond between metal and non metal is called

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

40.
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.
41.

Metallic bonding is...

a)

a type of covalent bond.

b)

a type of ionic bond.

c)

an attraction between positive ions and a "sea" of delocalised electrons.

42.
Ionic or covalent?
H2O
a)
Ionic
b)
Covalent
43.
Ionic or covalent?
NaBr
a)
Ionic
b)
Covalent
44.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
45.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
46.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

47.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

48.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

49.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

50.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

51.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
52.

What is the correct shape of CHCl3?

a)

Bent

b)

Trigonal pyramidal

c)

Tetrahedral

d)

Trigonal planar

53.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

54.

Conducts electricity when molten or aqueous

a)
ionic compound
b)
covalent compound
55.

After solute is added and the solution is stirred, some solute still remains undissolved. The solution is __________.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

56.

You can make a solute dissolve more quickly in a solvent by

a)

adding more solute.

b)

decreasing the the temperature

c)

increasing the temperature

d)

removing some solvent.

57.
This solution would be considered
a)
Unsaturated
b)
Supersaturated
c)
Saturated
d)
Undefined
58.
This graph represents a(n) ___ solution
a)
saturated
b)
supersaturated
c)
unsaturated
d)
undefined
59.

You add salt to a beaker of saltwater solution. The salt dissolves. The original solution was:

a)

Saturated

b)

Unsaturated

c)

Supersaturated

60.

You add solute to a solution and it crystallizes. The solution was:

a)

Saturated

b)

Unsaturated

c)

Supersaturated

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