PRACTICE - TEST on Atomic Structure
Name: ______________________
1) Complete the table below – Note that the particles are not is the same order: 3 points
Charge
Location
AMU
0
In Nucleus
1
Neutron
1Electron Cloud
0
Electron
1+
In Nucleus
1
Proton
2) Complete the table below -- 5 points
Isotope
Symbol
Protons + Neutrons = Mass #
Element
Name
Atomic
Number
Number of
Protons
Number of
Neutrons
Mass
Number
Number of
Electrons
15
N
Nitrogen
7
7
8
15
7
28
Al
Aluminum
13
13
15
28
13
41
Ca
Calcium
20
20
21
41
20
Bromine
35
35
39
74
35
74
Br
3) Complete the table below -- 5 points
F
P
Mg
N-m
N-m
M
Atomic #
9
15
12
P+
e-
9
15
12
9
15
12
E1 E2 E3 E4 Ve2
2
2
7
8
8
7
5
2
5
2
Group
7A - Halogens
5A 2A – Alkali Earth Metals
4) Draw the Lewis Structures for the following neutral atoms. 6 points
C
F
Si
He
Ga
Ba
5) Complete the boxes below. Be sure to include the electron configuration on the correct energy
levels. Draw the Lewis Structure of each resulting atom. 7 points
Oxygen - 16
Argon - 40
-
e
P+ = _8__
N0 = _8___
=
8_
2 6
1
2
Lewis
Structure
O
e- _18_
Lewis
Structure
288
Ar
P+ = _18__
N0 = _22__
1
3
Atomic # _8__ Mass # __16_
2
3
Atomic # _18__ Mass # _40_
6) What is the electron configuration of the following elements? (USE 1s2, 2s2…. Configuration)
3 points
Mg- 1s2, 2s2 , 2p6 , 3s2
(2, 8, 2)
Br- 1s2, 2s2 , 2p6 , 3s2 , 3p6 , 4s2, 3d10, 4p5
(2, 8, 18, 7)
Ag- 1s2, 2s2 , 2p6 , 3s2 , 3p6 , 4s2, 3d10, 4p6 , 5s2, 4d9 (2, 8, 18, 17, 2) -- actually (2,8,18,18,1)
E1=2, E2=2+6=8,
E3= 2+6+10 = 18,
E4 =2+6+9 = 17,
E5=2
7) Fill in the blanks using one of the following elements. Please note that each element may be used
once, more than once, or not at all. 10 points
K, Ca, Ga, C, As, O, Cl, Kr
__K, Ca, Ga__ is an example of metal
__ C, O, Cl, Kr _ is an example of a nonmetal
__ As ___ is an example of a metalloid
___O___ has an atomic number of 8
__ C ____ has 6 total electrons
__ O_ ___ has 6 valence electrons
__ K ____ has 1 valence electrons
___K___ has 19 protons
__ K, Ca, Ga, As,Kr _ is in period 4
__ Ca ___ is in period 2
__ As ___ is in group 5A
__ C ____ is in group 4A
__ Ca ___ is an Alkaline Earth Metal
__ Kr ___ is a Nobel Gas.
__ Cl __ is a Halogen
___ K __is an Alkali Metal
8) Look at each pair of elements below, select (circle) which element has the larger atomic radii:
Be or Ca
Na or P
N or B
3 points
9) Look at each pair of elements below, select (circle) which element has the higher ionization energy:
C or Si
F or Br
N or Li
3 points
10) Look at each pair of elements below, select (circle) which element has the higher electronegativity:
O or Se
P or Mg
N or F
3 points
11) TRUE or FALSE - there is no such thing as a 2p orbital.
12) TRUE or FALSE - the 3d orbital can hold a maximum of 6 electrons
13) TRUE or FALSE - electrons can be found between the energy levels (between E2 & E3 = E 2.5)
Moving from left-to-right across a period (row) of the periodic table,
14)
15)
16)
17)
18)
19)
TRUE or FALSE - the atomic mass increases by ONE from element to element (atomic number)
TRUE or FALSE - the elements become more non metallic
TRUE or FALSE - the ionization energy of the elements generally decreases
TRUE or FALSE - the elements are arranged according to increasing atomic number
TRUE or FALSE - each element has a unique number of neutrons
TRUE or FALSE - the atomic radius of the elements generally decreases
Directions: Match each item (a-p) with the correct statement below (16-31).
NOTE: Each item may be used once, more than once, or not at all.
a
b.
c.
d.
e.
atom
proton
neutron
electron
nucleus
f.
g.
h.
i.
j.
atomic number
atomic mass
mass number
isotope
atomic mass unit
k.
m.
n.
o.
p.
group
period
electronegativity
ionization energy
atomic radius
20. _a__ the smallest particle of an element that retains the properties of that element
21. _k__ vertical column in the periodic table
22. _h__ the total number of protons and neutrons in the nucleus of an atom
23. _b__ the identity of an element is determined by the number of ___________ in the nucleus
24. _p__ one-half the distance between the nuclei of two atoms when the atoms are joined
25. _d__ a negatively charged subatomic particle
26. _b__ a positively charged subatomic particle
27. _g__ the weighted average of the masses of the isotopes of an element
28. _e__ the central part of an atom, containing protons and neutrons
29. _f__ the number of protons in the nucleus of an element
30. _i__ atoms with the same number of protons, but different numbers of neutrons in the nucleus
31. _o__ energy required to remove an electron from an atom
32. _m__ horizontal row in the periodic table
33. _n__ ability of an atom to attract electrons when the atom is in a compound
34. _c__ a subatomic particle with no charge
35. _e__ almost all of the mass of the atom is contained in the __________
36) Neon is in period _
2__, group
__8A __, has __10 __ protons, and is considered a ___Nobel
For the following questions, put your answer in the box
Gas
___ at the beginning of the question.
37)
_4 _ Use the periodic table to determine the number of electrons in a neutral atom of beryllium.
38)
_35_ Use the periodic table to determine the number of protons in an atom of bromine.
39)
_33_ What is the atomic number for an element with 35 neutrons and a mass number of 68?
40)
_13_ What is the mass number for a carbon atom that has 7 neutrons in its nucleus?
41)
_46_ How many neutrons are present in an atom of the isotope
42)
_8 _ How many electrons are in the highest occupied energy level of a neutral neon atom?
43)
_11_ How many protons are present in an atom of Na-23?
Sr ?
_D__ 44) Which of the following is true about subatomic particles?
a. Electrons have no charge and have almost no mass.
b. Protons are negatively charged and the lightest subatomic particle.
c. Neutrons have a negative charge and are the lightest subatomic particle.
d. Electrons have almost no mass compared to the protons
_A__ 45) All atoms are ____.
a. neutral, with the number of protons equaling the number of electrons
b. neutral, with the number of protons equaling the number of electrons, which is equal to
the number of neutrons
c. positively charged, with the number of protons exceeding the number of electrons
d. negatively charged, with the number of electrons exceeding the number of protons
_B__ 46) The nucleus of all atoms ____.
a. always has the same number of neutrons and is considered neutral
b. are positively charged because of the positive charge of the protons
c. are negatively charged because of the negative charge of the neutrons
d. are positively charged and it occupies the vast majority of the volume of the atom.
_B__ 47) The sum of the protons and electrons in an atom equals the ____.
a. atomic number
b. charge of the atom
c. atomic mass
d. mass number
_B__ 48) What does the number 11 in the name boron-11 represent?
a. the atomic number
c. the sum of the protons and electrons
b. the mass number
d. twice the number of protons
_A__ 49) Isotopes of the same element have different ____.
a. numbers of neutrons b. numbers of protons c. numbers of electrons
_B__ 50) All atoms of the same element have the same ____.
a. number of neutrons
b. number of protons
c. mass numbers
d. atomic numbers
d. mass
_C__ 51) What unit is used to measure weighted average atomic mass?
a. photons
b. picometers
c. amu
d. density
_A__ 52) Which of the following statements is NOT true?
a. Atoms of the same element must always have the same mass
b. Atoms of isotopes of an element have different numbers of neutrons.
c. The nucleus of an atom has a positive charge.
d. Atoms are mostly empty space.
_D__ 53) Which of the following would be an isotope of an element that had 17 protons, 18 neutrons
and 17 electrons?
a. 17 protons, 18 neutrons, 18 electrons
c. 18 protons, 18 neutrons, and 17 electrons
b. 17 protons, 18 neutrons, 16 electrons
d. 17 protons, 17 neutrons, and 17 electrons
_D__ 54) How many protons, electrons, and neutrons does an atom with atomic number 75 and mass
number 145 contain?
a. 50 protons, 50 electrons, 75 neutrons
c. 120 neutrons, 50 protons, 75 electrons
b. 75 electrons, 50 protons, 50 neutrons
d. 70 neutrons, 75 protons, 50 electron
_C__ 55) How do the isotopes Carbon-12 and Carbon-13 differ?
a. Carbon-12 has one more electron than hydrogen-1.
b. Carbon-12 has 12 neutrons; carbon-13 has 13 neutrons
c. Carbon-13 has one more neutron than carbon-12
d. Carbon-13 has one more proton that carbon-12
_D__ 56) The atomic mass of an element depends on the _______.
a. Mass of each electron in that element
b. Mass of each isotope of that element
c. Relative abundance of protons in that element
d. Mass and relative abundance of each isotope of that element
_C__ 57) In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a. position
b. color
c. energy
d. size
_B__ 58) How does the energy of an electron change when the electron moves farther from the nucleus?
a. It decreases.
b. It increases
c. It stays the same. d. It doubles.
_A__ 59) What is the maximum number of electrons in the first principal energy level (E1)?
a. 2
b. 8
c. 18
d. 32
_B__ 60) What is the number of electrons in the outermost energy level of an silicon atom?
a. 2
b. 4
c. 6
d. 8
_B__ 61) Emission of light from an atom occurs when an electron ____.
a. becomes excited and jumps to a higher energy level
c. is in its ground state
b. relaxes and returns to its ground state
d. is in its excited state
_D__ 62) Which of the following elements is in the same period as krypton?
a. helium
b. magnesium
c. nitrogen
d. bromine
_B__ 63) Who arranged the elements according to atomic mass and used the arrangement to predict
the properties of missing elements?
a. Henry Moseley
b. Dmitri Mendeleev
c. JJ Thomson
d. John Dalton
_B__ 64) Of the elements Fr, Sb, Al, and Rn, which is a metalloid?
a. Fr
b. Sb
c. Al
d. Rn
_B__ 65) Each period in the periodic table corresponds to ______.
a. the number of valence electrons b. energy levels c. the mass
d. protons and neutrons
_B__ 66) How does the atomic radius change from top to bottom in a group in the periodic table?
a. it tends to decrease
c. It first increases, then decreases
b. it tends to increase
d. It does not change, it will always be the same
omit 67) Which of the following increases (decreases) with increasing atomic number in Group 2A?
a. shielding effect
b. ionic size
c. ionization energy
d. number of electrons
_C__ 68) Which of the following orbitals has the highest amount of energy?
a. 3d
b. 4p
c. 4f
d. 5s
69) Explain how you can use the periodic table of elements to determine the number of electrons in the
outer most energy level. 3 points
The periodic table will tell you the number of protons and therefore the number of
electrons that a neutral atom has. By drawing a Bohr model of the atom, it is possible to
determine the number of valence electrons that an atom has.
OR
The group number (1A – 8A) is directly related to the number of valence electrons.
Group 2A has 2 valence electrons, group 6A has six valence electrons.
70) Why is the Bohr model of an atom more useful than the previous models of the atom? 3 points
The Bohr model includes energy levels. These energy levels allow us to
determine the number of valence electrons available for bonding for each
element. The Bohr model also provides the evidence of how light is created
when an excited electron relaxes back down to its ground state and releases
energy in the form of a photon (light).
71) Explain the process of electron excitation. 2 points
When additional energy is added to a ground state electron (via a photon,
heat, electricity…), this additional energy can cause the electron to
temporarily jump to a higher energy level (the excited state). This jump
from ground state to excited state (because of the additional energy) is
referred to as excitation.
72) Which elements have similar properties to the element Chlorine (Cl)? 2 points
F, Br, I, At
73) How do you know that these elements have similar properties to Chlorine? 2 points
All of these elements are in the same group/family (7A) and each has
seven valence electrons. By having the same number of valence
electrons, each element has similar properties.
74) Consider an element Z that has two naturally occurring isotopes with the following percent abundances:
the isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is
45.0% abundant. Calculate the average ATOMIC MASS for element Z. SHOW YOUR WORK
3 points
Mass
19.0
21.0
x Abundance
x
0.55
= 10.45 AMU
x 0.45
= 9.45 AMU
(Note: 55.0% = 0.55)
(Note: 45.0% = 0.45)
19. 90 AMU is the Atomic Mass for element Z