Download Unit #3: Atomic Structure Exam Review

Unit #3: Atomic Structure Exam Review:
1) The atomic number of an element is determined by the number of
_________Protons_________ in the nucleus of an atom.
2) The philosopher, ______Democritus_______, believed that all matter consisted of
extremely small particles that could not be divided. He called these particles
____Atoms____, which means “uncut” or “indivisible.”
3) ______Ernest Rutherford______ provided evidence for the existence of a nucleus.
4) Complete the following table:
Energy Levels:
Maximum Number of Electrons:
1
2
3
4
2
8
18
32
5) Complete the following table:
Region of
Location:
Charge:
the Atom:
Center of
Nucleus
Positive
the Atom
Electron
Around the
Negative
Cloud
Nucleus
6) Complete the following table:
Subatomic
Location:
Particle:
Proton
Neutron
Electron
Nucleus
Nucleus
Electron Cloud
Mass:
Volume:
Density
Large
Small
Large
Small
Large
Small
Charge:
Mass:
Positive
Neutral
Negative
1 amu
1 amu
0 amu
7) Complete the following table:
Subshell:
Maximum Number
of Electrons:
Number of Orbitals:
s
p
d
f
2
6
10
14
1
3
5
7
8) Give the electron configuration, orbital notation, and atomic structure for the following
elements:
a) Magnesium
1s22s22p63s2
1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓
)
)
)
2e-
8e-
2e-
12 p+
12 n
b) Chlorine
1s22s22p63s23p5
1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓ 3p↑↓ ↑↓ ↑_
17 p+
18 n
)
)
)
2e-
8e-
7e-
c) Potassium
1s22s22p63s23p64s1
1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓ 3p↑↓ ↑↓ ↑↓ 4s↑_
19 p+
20 n
)
)
)
)
2e-
8e-
8e-
1e-
d) Rubidium
1s22s22p63s23p64s23d104p65s2
1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓ 3p↑↓ ↑↓ ↑↓ 4s↑↓ 3d↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p↑↓ ↑↓ ↑↓ 5s↑↓
37 p+
48 n
)
)
)
)
)
2e-
8e-
18e-
8e-
1e-
9) Identify how many protons, neutrons, and electrons a neutral atom of Fluorine contains.
9 Protons, 10 Neutrons, 9 Electrons
10) Identify how many protons, neutrons, and electrons a neutral atom of Bismuth contains.
83 Protons, 126 Neutrons, 83 Electrons
11) Identify how many protons, neutrons, and electrons a neutral atom of Cesium contains.
55 Protons, 78 Neutrons, 55 Electrons
12) Identify the element symbol for the following elements:
a) Aluminum  Al
c) Potassium  K
b) Sodium  Na
d) Manganese  Mn
13) ______Neils Bohr______ believed that electrons move around the nucleus like planets
orbiting the Sun.
14) In a few sentences describe Ernest Rutherford’s famous gold-foil experiment.
Rutherford aimed a beam of alpha particles (Helium nuclei) at a sheet of gold-foil
surrounded by a fluorescent screen. Most of the particles passed through, a few
deflected. Rutherford concluded that atoms were made up of mostly empty space
because most particles passed through. The particles that came close to the nucleus
were deflected due to a central, positive charge.
15) _________J.J. Thomson_________ provided evidence for the existence of electrons.
16) ________Eugen Goldstein_______ provided evidence for the existence of protons.
17) ________James Chadwick_______ provided evidence for the existence of neutrons.
18) Identify the atomic number and mass number for Mercury.
Atomic Number = 80
Mass Number = 201
19) Identify the atomic number and mass number for Zinc.
Atomic Number = 30
Mass Number = 65
20) Identify the atomic number and mass number for Uranium.
Atomic Number = 92
Mass Number = 238
21) Using the periodic table, what is the average atomic mass for Calcium?
40.08 amu
22) Using the periodic table, what is the average atomic mass for Silver?
107.87 amu
23) Using the periodic table, what is the average atomic mass for Carbon?
12.011 amu
24) How do you determine the number of protons in an atom?
Number of Protons = Atomic Number
25) How do you determine the number of electrons in an atom?
Number of Electrons = Number of Protons
26) What is the equation that is used to calculate the number of neutrons in an atom?
Number of Neutrons = Mass Number – Atomic Number
27) An atom has 16 protons, 16 neutrons, and 16 electrons. What is the element’s atomic
number and mass number?
Atomic Number = 16
Mass Number = 32
28) Complete the following table:
Element
Element
Number of
Number of
Number of
Name:
Symbol:
Protons:
Neutrons:
Electrons:
Lithium
Li
3
4
3
Silicon
Si
14
14
14
Mercury
Hg
80
121
80
Nickel
Ni
28
31
28
Bromine
Br
35
45
35
Calcium
Ca
20
20
20
Argon
Ar
18
22
18
Magnesium
Mg
12
12
12
29) If the atom is neutral, then the number of protons is equal to the number of
________Electrons_________.
30) _______Mass Number_______ refers to the sum of protons and neutrons in the nucleus
of an atom.
31) An element’s ______Average Atomic Mass_________ is an average mass of the
different isotopes of an element.
32) _______Isotopes________ are atoms of the same element with different numbers of
neutrons.
33) ______Atomic Number_____ refers to the number of protons in the nucleus of an atom.
34) Define the following terms:
a) Aufbau Principle: Electrons must enter orbitals of lowest energy first; Chart of
Electron Filling.
b) Hund’s Rule: When electrons occupy orbitals of equal energy, one electron enters
each orbital until all the orbitals contain one electron with parallel spins.
c) Pauli Exclusion Principle: Atomic orbitals may describe at most two electrons and
they must have an opposite spin.
d) Average Atomic Mass: Weighted average mass of the atoms in a naturally occurring
sample of an element.
e) Protons: Positively charged subatomic particle that is found in the nucleus, and has a
mass of 1 amu.
f) Neutrons: Neutral subatomic particle that is found in the nucleus, and has a mass of
1 amu.
g) Electrons: Negatively charged subatomic particle that is found in the electron cloud,
and does not have a mass.
h) Isotope: Atoms of the same element with a different number of neutrons, therefore
they have a different mass.
i) Element: Substance that cannot be broken down into simpler substances; Contains
only one type of atom.
j) Atomic Number: Number of protons in the nucleus of an atom; This number
identifies the element.
k) Mass Number: Sum of the protons and neutrons in the nucleus of an atom.
l) Nucleus: Dense, positively charged region that is located in the center of an atom;
Contains protons and neutrons.
m) Electron Cloud: Negatively charged region that surrounds the nucleus of an atom;
Contains electrons.
n) Electron Cloud Model: Visual model of the most likely locations for electrons in an
atom.
o) Energy Levels: Similar energies that electrons in an atom can have.
p) Subshells: Energy level that contains electrons that have the same energy.
q) Compound: Substance that is made from two or more simpler substances and can
be broken down into those simpler substances.