WorksheetsSemester Exam Review
Total questions: 40
Worksheet time: 40mins
Name
Class
Date
1.
Which of the following represents the correct electron configuration for chlorine (Cl)?
a)
A. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4p^6 5s^2
b)
B. 1s^2 2s^2 2p^6 3s^2 3p^5
c)
C. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1
d)
D. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4p^5
2.
What is the name of the compound with the formula PCl5?
a)
A. Phosphorus chloride
b)
B. Phosphorus pentachloride
c)
C. Phosphorus chlorate
d)
D.Phosphorus pentoxide
3.
a)
A
b)
B
c)
C
d)
D
4.
An element has two isotopes with masses of 10 amu and 11 amu. If their abundances are 70% and 30%, respectively, what is the average atomic mass?
a)
A. 10.1 amu
b)
B. 10.3 amu
c)
C. 10.5 amu
d)
D. 10.7 amu
5.
Henry, David, and Ethan are having a debate about chemistry. They are stuck on a question and need your help. Can you tell them what is the intermolecular force in NH3?
a)
dipole-dipole
b)
london dispersion force
c)
hydrogen bonding
d)
ionic bond
6.
What is the electron dot structure for oxygen (O)?
a)
A
b)
B
c)
C
d)
D
7.
Imagine Lily, Benjamin, and Aiden are playing a game of 'Guess the Element' in their chemistry class. Lily picks an element and gives a clue: 'My element is essential for life and its atomic number is the same as the number of legs on an octopus.' What is the atomic number of Lily's element?
a)
32
b)
16
c)
4
d)
8
8.
What are oxyacids?
a)
Acids that contain oxygen atom(s)
b)
Acids that do not contain oxygen atom(s)
c)
Acids that are only found in living organisms
d)
Acids that are only found in rocks and minerals
9.
Which of the following statements is true about ionic compounds?
a)
They are formed by the transfer of electrons between atoms.
b)
They consist of hydroxide ions held together by electrostatic forces.
c)
They involve the sharing of electrons between atoms.
d)
It has two types (polar and nonpolar)
10.
What did the Bohr model assume about the motion of electrons?
a)
All electrons move in a circular orbit around the nucleus.
b)
Electrons do not have a specific path around the nucleus.
c)
All electrons move in a single cloud layer around the nucleus.
d)
Electrons always remain in the same location around a nucleus.
11.
Atoms have positively charged particles, negatively charged particles, and particles with no charge. Why is an atom electrically neutral?
a)
Atoms have the same number of electrons (negative charge) and protons (positive charge).
b)
An atom’s nucleus has only neutrons, which have no charge.
c)
Atoms contain subatomic particles and not electrically charged particles.
d)
Atoms have neutrons and protons in the nucleus, and they do not have a charge.
12.
During a lab, a student stirs crushed ice into warm water. What assumption can the student make about the second law of thermodynamics?
a)
The ice cubes lose heat and the warm water gains heat until the temperature in the system is uniform throughout.
b)
The ice cubes gain heat and the warm water loses heat until the temperature in the system is uniform throughout.
c)
Both the ice cubes and the warm water lose heat, and thermal equilibrium is not reached.
d)
Both the ice cubes and the warm water gain heat, and thermal equilibrium is not reached.
13.
What is always the direction of heat transfer?
a)
From an object of greater mass to an object of less mass
b)
From an object with greater thermal energy to an object with less thermal energy
c)
From an object with less thermal energy to an object with greater thermal energy
d)
From matter at higher temperature to matter at lower temperature
14.
The subatomic particle with a negative charge is the ...
a)
electron
b)
proton
c)
neutron
d)
ion
15.
How do endothermic reactions impact the overall kinetic energy of the molecules? Select all that apply.
a)
An endothermic reaction reduces the average kinetic energy of the molecules in the reaction mixture (the surroundings).
b)
Energy is released during an endothermic reaction.
c)
An endothermic reaction increases the average kinetic energy of the molecules in the reaction mixture (the surroundings).
16.
Consider the scenario in which you are sitting by the campfire on a cold night. Which description best summarizes the heat transfer that occurs?
a)
The burning of the wood absorbs energy from its surroundings. Heat is transferred from your body to the campfire.
b)
The burning of the wood releases energy to its surroundings. Heat is transferred from the campfire to your body.
c)
The heat released by the campfire is balanced by the heat absorbed from its surroundings, so that the heat flow out of the system equals the heat flow into the system.
d)
Heat does not flow between the campfire and your body, as thermal equilibrium already has been achieved.he molecules in the reaction mixture (the surroundings).
17.
How many electrons does one neutrally charged atom of argon have?
a)
22
b)
18
c)
40
d)
58
18.
How many neutrons are there in Radium?
a)
88
b)
138
c)
226
d)
314
19.
What is the lowest possible energy level that an electron can occupy?
a)
ground state
b)
excited state
c)
fundamental state
d)
outermost state
20.
How many electrons are located in the outermost orbit in the Bohr model of a boron atom?
a)
1
b)
2
c)
3
d)
4
21.
The electron shell model of an atom has three main components: the energy shell, the subshell, and the orbital. Which of the following represent the correct arrangement from the lowest to highest maximum capacity to hold electrons?
a)
orbitals < energy shell < subshell
b)
energy shell < orbitals < subshell
c)
subshell < orbitals < energy shell
d)
orbitals < subshell < energy shell
22.
Consider the electron configuration of sulfur. How many unpaired electrons does sulfur have?
a)
2
b)
1
c)
3
d)
4
23.
The atomic number of an element is 15. What is the likely electron configuration arrangement of the valence and core electrons in a neutral atom of this element?
a)
There are 3 valence electrons and 12 core electrons.
b)
There are 4 valence electrons and 11 core electrons.
c)
There are 5 valence electrons and 10 core electrons.
d)
There are 6 valence electrons and 9 core electrons.
24.
An atom of chlorine has 17 electrons. These electrons are present in energy shells around the nucleus. Which series of numbers lists the correct number of electrons in each energy shell, starting with the energy shell closest to the nucleus?
a)
2,8,1
b)
2,8,7
c)
2,8,17
d)
2,10,5
25.
The valence electrons of an atom do not experience the full attractive force of protons in the atom’s nucleus due to the presence of inner core electrons. The reduction in nuclear charge experienced by valence electrons due to inner core electrons is called the .....
a)
ionization energy effect.
b)
nuclear charge effect
c)
periodic law effect.
d)
shielding effect.
26.
Name two elements that have similar properties based on their groupings in the periodic table.
a)
Li and O
b)
Na and Li
c)
B and Cl
d)
O and Cl
27.
How are the elements in today’s modern periodic table arranged?
a)
in order of increasing atomic number
b)
in order of decreasing atomic number
c)
in order of increasing atomic mass
d)
in order of decreasing atomic mass
28.
From left to right across a period for main-group elements, the effective nuclear charge
a)
increases.
b)
decreases.
c)
remains the same.
d)
increases and then decreases.
29.
Which of the following elements is found in group 2, period 3 of the periodic table?
a)
boron
b)
calcium
c)
aluminum
d)
magnesium
30.
How many valence electrons are lost by the metallic element when forming the ionic compound BaS?
a)
1
b)
2
c)
3
d)
4
31.
What is the maximum number of electrons in the fourth energy level?
a)
32 electrons
b)
18 electrons
c)
6 electrons
d)
2 electrons
32.
What is the electron configuration for sulfur?
a)
1s2 2s2 2p4 3s2 3p6
b)
1s2 2s2 2p4 3s2 3p10
c)
1s2 2s2 2p6 3s2 3p6
d)
1s2 2s2 2p6 3s2 3p4
33.
Which of the following correctly describes the structure of ionic compounds?
a)
individual molecules
b)
randomly arranged ions
c)
a crystal lattice
d)
free-floating atoms
34.
What property of ionic compounds is explained by their strong electrostatic interactions?
a)
low melting point
b)
high melting and boiling points
c)
flexibility
d)
weak electrical conductivity in liquid form
35.
Arrange the following elements in increasing number of electrons. (H,Ca,Ar,Se)
a)
H,Ar,Ca,Se
b)
H,Ca,Ar,Se
c)
Ar,Se,Ca,H
d)
Ca,Se,Ar,H
36.
Order the following atoms from highest to lowest number of protons (Sn,K,Ga,Ba,Al)
a)
Sn,K,Ga,Ba,Al
b)
Ba,Sn,Ga,Al,K
c)
Ba,Sn,Ga,K,Al
d)
Sn,Ba,Ga,K,Al
37.
Which of the following correctly completes the statement:
Cations are always _____ than the parent atom and anions are always _____ than the parent atom.
a)
smaller, smaller
b)
larger, smaller
c)
larger,larger
d)
smaller, larger
38.
Lithium is in Group 1A, Period 2 of the periodic table. Which statement describes the charge of the ion it typically forms?
a)
It forms a cation with +2 charge.
b)
It forms a cation with a -1 charge.
c)
It forms a cation with a +1 charge.
d)
It forms an anion with a −1 charge.
39.
Given the following elements with their ionization energies, which of these elements is most likely to be located at the top of its group?
- Elements: A (496 kJ/mol), B (2372 kJ/mol), C (1314 kJ/mol), D (577 kJ/mol)
a)
Element A
b)
Element B
c)
Element C
d)
Element D
40.
Which of the following factors primarily explains why atomic radii increase down a group?
a)
Increasing number of protons
b)
Decreasing number of electrons
c)
Addition of electron shells
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