Download TEST on Atomic Structure

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
Neutron
Electron
Proton
2) Complete the table below -- 5 points
Isotope
Symbol
Element
Name
15
N
Atomic
Number
Number of
Protons
Number of
Neutrons
Mass
Number
Nitrogen
Number of
Electrons
15
28
Al
Calcium
21
39
74
3) Complete the table below -- 5 points
Atomic #
F
P
Mg
P+
e-
E1 E2 E3 E4 Ve-
Group
N-m
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. 8 points
Oxygen - 16
Argon - 40
-
e
=
___
P+ = _____
N0 = _____
e- =____
Lewis
Structure
P+ = _____
N0 = _____
1
2
1
3
Atomic # ____ Mass # ____
2
3
Atomic # ____ Mass # ____
Lewis
Structure
6) What is the electron configuration of the following elements? (USE 1s2, 2s2…. Configuration)
3 points
MgBrAg-
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. 16 points
K, Ca, Ga, C, As, O, Cl, Kr
________ is an example of metal
________ is an example of a nonmetal
________ is an example of a metalloid
________ has an atomic number of 8
________ has 6 total electrons
________ has 6 valence electrons
________ has 1 valence electrons
________ has 19 protons
________ is in period 4
________ is in period 2
________ is in group 5A
________ is in group 4A
________ is an Alkaline Earth Metal
________ is a Nobel Gas.
________ is a Halogen
________ 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, (40-45
14)
15)
16)
17)
18)
19)
TRUE or FALSE - the atomic mass increases by ONE from element to element
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
average atomic mass
mass number
isotope
atomic mass unit
k.
m.
n.
o.
p.
group
period
electronegativity
ionization energy
atomic radius
20. ____ the smallest particle of an element that retains the properties of that element
21. ____ vertical column in the periodic table
22. ____ the total number of protons and neutrons in the nucleus of an atom
23. ____ the identity of an element is determined by the number of ___________ in the nucleus
24. ____ one-half the distance between the nuclei of two atoms when the atoms are joined
25. ____ a negatively charged subatomic particle
26. ____ a positively charged subatomic particle
27. ____ the weighted average of the masses of the isotopes of an element
28. ____ the central part of an atom, containing protons and neutrons
29. ____ the number of protons in the nucleus of an element
30. ____ atoms with the same number of protons, but different numbers of neutrons in the nucleus
31. ____ energy required to remove an electron from an atom
32. ____ horizontal row in the periodic table
33. ____ ability of an atom to attract electrons when the atom is in a compound
34. ____ a subatomic particle with no charge
35. ____ almost all of the mass of the atom is contained in the __________
36) Neon is in period _____, group ______, has _____ protons, and is considered a __________________
For the following questions, put your answer in the box
___ at the beginning of the question.
37)
___ Use the periodic table to determine the number of electrons in a neutral atom of beryllium.
38)
___ Use the periodic table to determine the number of protons in an atom of bromine.
39)
___ What is the atomic number for an element with 35 neutrons and a mass number of 68?
40)
___ What is the mass number for a carbon atom that has 7 neutrons in its nucleus?
41)
___ How many neutrons are present in an atom of the isotope
42)
___ How many electrons are in the highest occupied energy level of a neutral neon atom?
43)
___ How many protons are present in an atom of Na-23?
Sr ?
_____ 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
_____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
_____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.
_____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
_____ 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
_____ 49) Isotopes of the same element have different ____.
a. numbers of neutrons b. numbers of protons c. numbers of electrons
_____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
_____ 51) What unit is used to measure weighted average atomic mass?
a. photons
b. picometers
c. amu
d. density
_____ 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.
_____ 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
_____ 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
_____ 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
_____ 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
_____ 57) In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a. position
b. color
c. energy
d. size
_____ 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.
_____ 59) What is the maximum number of electrons in the first principal energy level (E1)?
a. 2
b. 8
c. 18
d. 32
_____ 60) What is the number of electrons in the outermost energy level of an silicon atom?
a. 2
b. 4
c. 6
d. 8
_____ 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
_____ 62) Which of the following elements is in the same period as krypton?
a. helium
b. magnesium
c. nitrogen
d. bromine
_____ 63) Electron configurations are arranged based upon_____?
a. the lowest possible energy
b. The number of protons in a neutral atom
c. the highest possible energy
d. The excitation and relaxation of the valence electrons
_____ 64) Of the elements Fr, Sb, Al, and Rn, which is a metalloid?
a. Fr
b. Sb
c. Al
d. Rn
_____ 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
_____ 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
_____ 67) Which of the following increases with increasing atomic number in Group 2A?
a. shielding effect
b. ionic size
c. ionization energy
d. number of electrons
_____ 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. 2 points
70) Explain the process of electron excitation. 2 points
71) Which elements have similar properties to the element Chlorine (Cl)? 2 points
72) How do you know that these elements have similar properties to Chlorine? 2 points
73) Consider an element Z that has two naturally occurring isotopes with the following percent abundances:
the isotope Z-19 with a mass number of 19.0 is 55.0% abundant; and the isotope Z-21 with a mass
number of 21.0 is 45.0% abundant. Calculate the average ATOMIC MASS for element Z. 3 points