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WorksheetsQ2 M1 - ELECTRIC STRUCTURE OF MATTER
Total questions: 69
Worksheet time: 28mins
Name
Class
Date
1.
On the basis of Rutherford’s model of an atom, which sub-atomic particle is present in the nucleus of an atom?
a)
proton only
b)
proton and electron
c)
proton and neutron
d)
neutron and electron
2.
If the first and second energy levels of an atom are full, then what would be the total number of electrons in the atom?
a)
6
b)
8
c)
10
d)
18
3.
Which atomic model is proposed by Schrodinger?
a)
nuclear model
b)
raisin bread model
c)
planetary model
d)
quantum mechanical model
4.
Which electron transition results in the emission of energy?
a)
1s to 2s
b)
2s to 2p
c)
3p to 3s
d)
3p to 4p
5.
The symbol “n” in the Bohr theory of atomic structure refers to the _______
a)
energy of electron
b)
total energy of the atom
c)
orbit in which an electron is found
d)
number of electrons in the energy level
6.
Which of the following sublevels is correctly designated?
a)
1p5
b)
2p6
c)
3f9
d)
3d11
7.
How many orbitals are in the third principal energy level?
a)
3
b)
6
c)
9
d)
12
8.
Which configuration is possible in an excited state of an electron?
a)
1H: 1d1
b)
11Na: 1s2 2s2 2p6 3d1
c)
2He: 1s2
d)
10Ne: 1s2 2s2 2p5 3s1
9.
What are the orbitals in the fifth principal energy level?
a)
s orbital
b)
s, p orbitals
c)
s, p, d orbitals
d)
s, p, d, f, and g orbitals
10.
For a neutral atom with the electron configuration of 1s2 2s2 2p5 3s1, which statement is FALSE?
a)
The atomic number is ten.
b)
The atom is in ground state.
c)
The atom is in an excited state.
d)
The 1s and 2s orbitals are filled.
11.
Rutherford’s model of the atom concentrated on the nucleus while Bohr’s model focused on the ______
a)
electrons
b)
protons
c)
neutrons
d)
quarks
12.
Which of the following statements about electrons refer to the Bohr Model of an atom?
a)
move at a very high velocity around the nucleus
b)
exist at different energy levels in orbit around the nucleus
c)
can move between energy levels when they gain or lose energy
d)
all of the above
13.
The following are rules/principles used in arranging the electrons around the nucleus of an atom EXCEPT
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
d)
Heisenberg’s Uncertainty Principle
14.
If a neutral atom has 18 electrons, what is the highest principal energy level that its outermost electrons will occupy?
a)
1
b)
2
c)
3
d)
4
15.
Which of the following is the correct electron configuration for neon (10Ne)?
a)
1s2 2s2 2p6
b)
1s4 2s2 3s2 2p2
c)
1s2 2s2 3s2 2p4
d)
1s2 2s2 3s1 2p5
16.
Who proposed the probability that electrons will be found in certain locations around the nucleus of an atom?
a)
Neils Bohr
b)
Erwin Schrodinger
c)
Ernest Rutherford
d)
J.J. Thomson
17.
Which of the following statements is NOT TRUE of the atomic model of Bohr?
a)
An electron can absorb or emit a quantity of radiation.
b)
The energy of the electron in a given orbit is not fixed.
c)
The hydrogen is made up of a positively charged nucleus.
d)
The electron revolves around the nucleus in a circular orbit.
18.
Which orbital designation has the highest energy?
a)
2s
b)
2p
c)
3s
d)
3d
19.
Which statement is INCORRECT?
a)
Orbital is a region in an atom where an electron can be found.
b)
An electron can emit energy when it jumps to a higher energy level.
c)
An electron can absorb energy when it jumps to a higher energy level.
d)
Filling of electrons in an atom starts from the low energy level to the highest energy level.
20.
What occurs when an electron moves from a high energy level to a low one?
a)
The atom moves faster.
b)
Colored light is given off.
c)
Colored light is absorbed.
d)
Another electron goes from a low energy level to a high one
21.
Which combination describes the flame color of the compound when heated?
a)
boric acid- red
b)
copper (II) sulfate- violet
c)
potassium chloride- blue
d)
sodium chloride- yellow orange
22.
What happens to the energy of an electron if it moves from one energy level to another closer to the nucleus?
a)
stays constant
b)
gains energy
c)
becomes an ion
d)
loses energy
23.
Which principle states that electrons occupy orbitals of lowest energy first before filling in the higher energy levels?
a)
Hund’s Rule
b)
Schrodinger’s Equation
c)
Aufbau Principle
d)
Pauli Exclusion Principle
24.
What shape are p orbitals?
a)
cloverleaf shaped
b)
hybrid structure
c)
dumbbell shaped
d)
spherical shape
25.
The exponent (superscript) in an electron configuration such as in 2p5 tells us the _____
a)
number of positions in that orbital
b)
distance from the nucleus or level
c)
number of electrons of that orbital
d)
number of electrons in the nucleus
26.
During a flame test, a copper (II) salt produces a bluish green color of flame. This color is produced when electrons in the excited copper II atoms _____
a)
are lost by the atoms
b)
are gained by the atoms
c)
move to higher energy states within the atoms
d)
return to lower energy states within the atoms
27.
Which of the following best describes the quantum mechanical model of the atom?
a)
It is the currently accepted atomic model.
b)
It was based on Schrodinger’s mathematical calculations.
c)
It describes an electron probability distribution through orbitals.
d)
all of the above
28.
The f orbitals can have how many orientations?
a)
1
b)
3
c)
5
d)
7
29.
Which electron movement is accompanied by a release of energy?
a)
1s to 2s
b)
2s to 2p
c)
3p to 3s
d)
4px to 4pz
30.
Which of the following statements about the orbital is FALSE?
a)
It can be unoccupied.
b)
It can be occupied by one electron.
c)
It can be occupied by two electrons.
d)
It can be occupied by more than two electrons.
31.
He proposed that the electron (which is also thought as a particle) could also be a wave.
(a)
32.
He used Broglie’s idea to develop a mathematical equation to describe the hydrogen atom.
(a)
33.
He discovered that for a very small particle like the electron, its location cannot be exactly known and how it is moving. This is called the uncertainty principle.
(a)
34.
Also known as electronic structure, is the arrangement of electrons in energy levels around an atomic nucleus.
(a)
35.
It states that in the ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels.
(a)
36.
It states that no two electrons in the same atom can occupy the same orbital and the two electrons in the same orbital must have opposite spins.
(a)
37.
No two electrons can be identified by the same set of quantum numbers.
(a)
38.
Bohr’s atomic model describes the atom like a solar system, where the electron is found only in specific circular paths, or orbits, around the nucleus.
a)
TRUE
b)
FALSE
39.
The quantum mechanical model of the atom describes the atom as having a nucleus at the center around which the electrons move. This model describes a region in space where the electron is most likely to be found.
a)
TRUE
b)
FALSE
40.
The way in which electrons are distributed in the different orbitals around the nucleus of an atom is called the electron configuration. Filling the electrons starts from the highest energy level to the lower energy level.
a)
TRUE
b)
FALSE
41.
The symbol “n” in the Quantum Mechanical Model of atomic structure refers to
a)
The orbit on which the electron is found
b)
The number of electrons in an energy level
c)
The total number of an atom
d)
The energy of an electron
42.
If the 1st and 2nd energy are full, then what would be the total number of electrons in the atom?
a)
6
b)
19
c)
10
d)
18
43.
How many orbitals are there in the 3rd energy level?
a)
9
b)
2
c)
3
d)
6
44.
Which of the properties of atoms is the most suitable reference for the kind of bond that will take place between/among them?
a)
Atomic size
b)
ionization energy
c)
Electronegativity
d)
electron affinity
45.
Among the following, the element that is not a noble gas is
a)
Ne
b)
Ar
c)
Xe
d)
U
46.
How many valence electrons do noble gases have?
a)
2
b)
4
c)
6
d)
8
47.
Cesium is located at period 7, family 1A in the periodic table of elements. It is the element with the highest ionization energy. How many valence electrons does Cs have?
a)
1
b)
2
c)
6
d)
7
48.
Which of the following sublevels is correctly designated?
a)
3d¹¹
b)
2f¹⁰
c)
1s⁴
d)
4p⁶
49.
How many orbitals are there in the 2nd principal energy level?
a)
1
b)
4
c)
9
d)
16
50.
Which configuration is possible in an excited state of an electron?
a)
2He 1s²
b)
10Ne 1s² 2s² 2p 3d¹
c)
1H 1d¹
d)
11Na 1s² 2s² 2p 3s¹
51.
What are the orbitals present in the fifth principal energy level?
a)
S orbital
b)
s, p, d orbitals
c)
S, p orbital
d)
s, p, d, and f orbitals
52.
For a neutral atom with the electron configuration of 1s² 2s² 2p 3s¹, which statement is false?
a)
The atom is in the ground state
b)
The atom is in the excited state
c)
The atomic number is 10
d)
The 1s and 2s orbitals are filled
53.
How are the electrons being arranged around the atoms?
a)
From a lower energy level to the highest energy level
b)
From the highest energy level to the lowest energy level
c)
From the 2nd energy level to the 1st energy level
d)
From the lowest energy level to the middle
54.
Which orbital designation has the highest energy?
a)
2s
b)
2p
c)
3d
d)
4s
55.
How many valence electrons do noble gases like Ne have?
a)
6
b)
4
c)
10
d)
8
56.
Cesium is located at period 7, Family 1A in the periodic table of elements. It is the element with the highest ionization energy. How many valence electrons do Cs have?
a)
2
b)
1
c)
5
d)
3
57.
What should be the electronic configuration of Ne?
a)
1s²2s² 2p²
b)
1s²2s² 2p⁴
c)
1s²2s² 2p⁶
d)
1s²2s² 2p
58.
What information is given by the principal quantum number of an electron?
a)
The orientations of the orbitals occupied by the electrons
b)
The type of orbital occupied by the electron.
c)
The spinning motion of the electron.
d)
The main energy level where the electron is located.
59.
What is the correct electronic configuration of the atom of an element whose atomic number is equal to 10?
a)
1s² 2s² 2p⁶
b)
1s² 2s² 2p 3s⁴
c)
1s² 2s² 2p 3s¹
d)
1s² 2s² 2p
60.
The symbol n in the Bohr Theory of atomic structures refers to
a)
The energy of the electron
b)
The total energy of the atom
c)
The orbit in which the electron is found
d)
The number of electrons in an energy level
61.
For a neutral atom with the electron configuration of 1s² 2s² 2p 3s¹, which statement is FALSE?
a)
the atomic number is 10
b)
the 1s and 2s orbitals are filled
c)
the atom is in the ground state
d)
the atom is in the excited state
62.
Which of the properties of atoms is the most suitable reference for the kind of bond that will take place between/among them?
a)
Atomic size
b)
Electronegativity
c)
ionization energy
d)
electron affinity
63.
What are the orbitals present in the fifth principal energy level?
a)
S orbital
b)
s, p orbitals
c)
s, p, d orbitals
d)
s, p, d, and f orbitals
64.
Which of the following is a metal?
a)
O
b)
S
c)
K
d)
C
65.
Which of the following designations has the highest energy?
a)
4s
b)
2p
c)
2s
d)
3d
66.
Which statement is incorrect?
a)
orbital is a region in an atom where an electron can be found
b)
an electron can emit energy when it jumps to a higher energy level
c)
an electron can absorb energy when it jumps to a higher energy level
d)
filling of electrons in an atom starts from a low energy level to the highest energy level
67.
What occurs when an electron moves from a high energy level to a low one?
a)
this process is not possible
b)
the atom moves faster
c)
another electron goes from a low energy level to a high one
d)
colored light is given off
68.
Which orbital designation has the highest energy?
a)
2s
b)
2p
c)
3d
d)
4s
69.
What are the orbitals present in the fifth principal energy level?
a)
S orbital
b)
S, p orbital
c)
s, p, d orbitals
d)
s, p, d, and f orbitals
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