Chapter 5 Quiz:
Name:
1) Help Jim out and write the symbol of a species that would be an example of each of
the following (use a different element each time):
a) non-metal
b) semi-metal
c) metal
d) alkali metal
e) alkaline earth metal
f) halogen
g) noble gas
h) ion
i) anion
j) cation
k) transition metal
l) lanthanide or actinide
2) WWE Elemental Smackdown!!! When she’s not studying chemistry, Emma loves to
watch professional wrestling.
9F
versus
87Fr
Compare the two elements above by writing the symbol of the appropriate
element in each blank.
a) higher first ionization energy
b) larger atomic radius
c) higher electronegatvity
d) higher electron affinity
e) non-metal
3) Use each of the following terms to explain each of the trends below to Lwam:
attraction
energy level effective nuclear charge
repulsion
a) Do atoms get bigger or smaller as you move down a group? Why?
b) Do atoms get bigger or smaller as you move to the right across a period? Why?
c) Are negative ions larger or smaller than the corresponding atoms? Why?
d) Are positive ions larger or smaller than the corresponding atoms? Why?
4) Sam is brimming over with curiosity about the reactivity of metals and non metals.
a) What is an example of a highly reactive metal? Explain this element’s high
reactivity in terms of electron configuration, valence electrons and periodic properties.
b) What is an example of a highly reactive non-metal? Explain this element’s high
reactivity in terms of electron configuration, valence electrons and periodic properties.
5) For each of the following, circle the equation that shows the process that is occurring,
and indicate whether it is exothermic or endothermic. Sophie would like to know.
a) first ionization of Mg
Mg
+
e-
=>
Mg-1
Exothermic
Mg
or
=>
Mg+1 +
e-
Endothermic
b) electron affinity of Cl
Cl
+
e-
=>
Cl-1
Exothermic
Cl
or
=>
Cl+1
Endothermic
+
e-
6) For each of the following elements, write the electron configuration, the number of
valence electrons, and the most common charge the element would have as an ion.
Electron Configuration
# Valence Electrons Charge
Na
Ca
Al
S
F
7) For each of the following pairs, circle the ion or atom with the smallest radius.
a) Cl
Ar
b) Ar
Kr
c) Cl
Cl-1
d) K
K+1
e) Cl
K
8) Using the symbols < and > in each of the blanks, indicate which of the following is the
larger quantity in each of the following pairs. For part c, please explain your answers to
parts a and b in a manner that Trilok would understand.
a) first ionization energy of Na _____ first ionization energy of Mg
b) second ionization energy of Na _____ second ionization energy of Mg
c)
_____9) Which Group of the Periodic Table contains atoms with a stable outer electron
configuration?
(1) 1
(3) 16
(2) 8
(4) 18
_____10) From which of these atoms in the ground state can a valence electron be removed using
the least amount of energy?
(1) nitrogen
(3) oxygen
(2) carbon
(4) chlorine
_____11) Which statement best describes electrons?
(1) They are positive subatomic particles and are found in the nucleus.
(2) They are positive subatomic particles and are found surrounding the nucleus.
(3) They are negative subatomic particles and are found in the nucleus.
(4) They are negative subatomic particles and are found surrounding the nucleus.
_____12) The strength of an atom’s attraction for the electrons in a chemical bond is the atom’s
(1) electronegativity
(3) heat of reaction
(2) ionization energy
(4) heat of formation
_____13) Given the equation:
This equation represents the formation of a
(1) fluoride ion, which is smaller in radius than a fluorine atom
(2) fluoride ion, which is larger in radius than a fluorine atom
(3) fluorine atom, which is smaller in radius than a fluoride ion
(4) fluorine atom, which is larger is radius than a fluoride ion
_____14) Which list of elements contains two metalloids, or semimetals?
(1) Si, Ge, Po, Pb
(3) Si, P, S, Cl
(2) As, Bi, Br, Kr
(4) Po, Sb, I, Xe
_____15) What is the total number of electrons in a Cu+1 ion?
(1) 28
(3) 30
(2) 29
(4) 36
_____16) Which list of elements is arranged in order of increasing atomic radii?
(1) Li, Be, B, C
(3) Sc, Ti, V, Cr
(2) Sr, Ca, Mg, Be
(4) F, Cl, Br, I
_____17) Which ion has the same electron configuration as an atom of He?
(1) Be+2
(3) Na1+
2–
(2) O
(4) Ca2+
_____18) What is the total number of valence electrons in an atom of sulfur in the ground state?
(1) 6
(3) 3
(2) 8
(4) 4
_____19) What occurs when an atom of chlorine forms a chloride ion?
(1) The chlorine atom gains an electron, and its radius becomes smaller.
(2) The chlorine atom gains an electron, and its radius becomes larger.
(3) The chlorine atom loses an electron, and its radius becomes smaller.
(4) The chlorine atom loses an electron, and its radius becomes larger.
_____20) In which group of the Periodic Table do most of the elements exhibit both positive and
negative oxidation states, or charges?
(1) 15
(3) 18
(2) 2
(4) 7
_____21) The element in Period 4 and Group 1 of the Periodic Table would be classified as a
(1) metal
(3) nonmetal
(2) metalloid or semimetal
(4) noble gas
_____22) As the elements in Period 2 of the Periodic Table are considered in succession from left
to right, there is a decrease in atomic radius with increasing atomic number. This may best be
explained by the fact that the
(1) number of protons increases, and the number of shells (or energy levels) of electrons remains
the same
(2) number of protons increases, and the number of shells of electrons increases
(3) number of protons decreases, and the number of shells of electrons remains the same
(4) number of protons decreases, and the number of shells of electrons increases
_____23) Which particle has the same electron configuration as a potassium ion?
(1) fluoride ion
(3) neon atom
(2) sodium ion
(4) argon atom
_____24) A neutral atom contains 12 neutrons and 11 electrons. The number of protons in this
atom is
(1) 1
(3) 12
(2) 11
(4) 23
_____25) Which element is a noble gas?
(1) krypton
(3) antimony
(2) chlorine
(4) manganese
_____26) The amount of energy required to remove the outermost electron from a gaseous atom
in the ground state is known as
(1) first ionization energy
(2) electron affinity
(3) conductivity
(4) electronegativity
_____27) What is a property of most metals?
(1) They tend to gain electrons easily when bonding.
(2) They tend to lose electrons easily when bonding.
(3) They are poor conductors of heat.
(4) They are poor conductors of electricity.