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Semester 1 final review( 2025 -26)

Total questions: 40

Worksheet time: 35mins

Name
Class
Date
1.

What is the formula for sodium sulfate?

a)

Na2(SO4)

b)

Na(SO4)2

c)

Na(SO4)

d)

Na2(SO4)2

2.

Molecular compounds are usually_______

a)

composed of two or more transition elements

b)

composed of positive and negative ions

c)

composed of two or more nonmetallic elements

d)

exceptions to the law of definite proportions

3.

What is the ending for the names of all binary compounds, both ionic and molecular?

a)

ate

b)

ite

c)

ide

d)

ade

4.

Which of the following formulas represents a molecular compound?

a)

ZnO

b)

Xe

c)

BeF2

d)

so2

5.

How many molecules are in 2.10 mol CO2?

a)

1.26 x 1024 molecules

b)

1.26 x 1023 molecules

c)

3.26 x 1024 molecules

d)

2.26 x 1023 molecules

6.

What is the mass of silver in 3.4 g AgNO3?

a)

2.2 g

b)

3.0 g

c)

0.64 g

d)

.025 g

7.

Which element, when combined with fluorine, would most likely form an ionic compound?

a)

Carbon

b)

Phosphorous

c)

Lithium

d)

Chlorine

8.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
9.
C4H12 + O2 → CO2 + H2O
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
10.
__H2O2 --> __H2O + __O2
a)
already balanced
b)
2,1,1
c)
2,2,1
d)
2,1,2
11.
_AgNO3 + _Cu →_Cu(NO3)2 + _Ag
a)
2 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 1 Ag
b)
2 AgNO3 + 1 Cu → 1 Cu(NO3)2 + 2 Ag
c)
1 AgNO3 + 2 Cu → 2 Cu(NO3)2 + 1 Ag
d)
3 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 2 Ag
12.

An atom with 1 valence electron 'needs' a full shell, so it can either gain 7 electrons or lose 1. Which is more likely to occur?

a)

nothing

b)

gain 7

c)

lose 1

13.

How are ionic bonds formed?

a)

transfer of electrons

b)

sharing of electrons

14.

Group numbers on the periodic table help us determine

a)

number of valence electrons

b)

state of the element (solid, liquid, gas)

15.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
16.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
17.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
18.
Which has the greater EN: 
H or F?
a)
H
b)
F
19.
Put these in increasing order:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
20.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
21.

Why does atomic size increase down a group?

a)

the atom is adding energy levels

b)

the atom is adding protons and electrons so more attraction

c)

the atom is losing energy levels

22.

Why does atomic size decrease across a period?

a)

the atom is adding protons and electrons so less attraction and a new energy level is added

b)

the atom is adding protons and electrons so more attraction but no new energy level is added

c)

the atom is losing energy levels and has more attraction

23.

Why is Na atom larger than a Li atom?

a)

Na has one more energy level than Li

b)

Na has less electrons and protons than Li

c)

Na has one less energy level than Li

24.

Arrange the following elements in order of decreasing size; F, Li, Be, N, O

a)

Li, Be, N, O, F

b)

F, N, O, Be, Li

c)

F, Li, Be, N, O

25.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
26.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

27.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.


Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).

a)

Lithium and cadmium are in the mixture. Strontium is not in the mixture.

b)

Lithium and strontium are in the mixture. Cadmium is not in the mixture

c)

Cadmium and strontium are in the mixture. Lithium is not in the mixture

d)

All of the shown elements are present in the mixture.

28.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
29.

Which element has the smallest atomic radius among B, N, and F?

a)

Boron (B)

b)

Nitrogen (N)

c)

Fluorine (F)

30.

What is the main factor that determines the chemical reactivity of an element in the periodic table?

a)

Density

b)

Number of neutrons

c)

Atomic mass

d)

Number of valence electrons

31.

Which of the following best describes a covalent bond?

a)

Transfer of electrons between atoms

b)

Sharing of electrons between atoms

c)

Formation of ions

d)

Loss of protons from the nucleus

32.

What is the trend in electronegativity as you move from left to right across a period in the periodic table?

a)

It first increases then decreases

b)

It remains the same

c)

It increases

d)

It decreases

33.

Which element has the smallest atomic radius among the following?

Li, Be, B, C

a)

Li

b)

Be

c)

B

d)

C

34.

What is the correct formula for calcium chloride?

a)

Ca2Cl

b)

CaCl

c)

CaCl2

d)

Ca2Cl2

35.

Which of the following molecules exhibits hydrogen bonding as its strongest intermolecular force?

a)

CH4

b)

CO2

c)

HCl

d)

NH3

36.

What is the correct name for the molecular compound N2O4?

a)

Tetranitrogen dioxide

b)

Nitrogen oxide

c)

Dinitrogen tetraoxide

d)

Nitrogen dioxide

37.

Which element has the highest ionization energy among the following?

Na, Mg, Al, P

a)

Na

b)

Mg

c)

Al

d)

P

38.

Which of the following elements has the highest electronegativity?

Li, Be, N, O

a)

Be

b)

O

c)

N

d)

Li

39.

What is the correct name for the molecular compound CO2?

a)

Dicarbon monoxide

b)

Monocarbon dioxide

c)

Carbon monoxide

d)

Carbon dioxide

40.

Which of the following best describes an ionic bond?

a)

Loss of neutrons from the nucleus

b)

Sharing of electrons between atoms

c)

Transfer of electrons from one atom to another

d)

Equal sharing of protons

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