Download Study Guide Chemistry Test #5

Study Guide
Chemistry Test #5
Learning Goals for Unit #5:
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To identify key info about elements including:
o Classification and state of matter at room temp
o Family names
o Valence electrons
o Tendencies to lose, gain or share electrons
o Special properties and whether or not they are found free in nature
To explain how reactivity changes within a group - most reactive vs least reactive
To define atomic radius and the factors that influence it
To define electronegativity, electron affinity and ionization energy and…
o To identify the trends throughout the periodic table
o To explain relationship to atomic radius and classification of element
To define ions and differentiate between ions and atoms
To identify how ionic radius is different from atomic radius for a given element
1) Who is credited with producing the first periodic table?
2) Who is credited with the concept of atomic number?
3) Why are the alkali metals more reactive than the Group 13 metals? Use key terms.
4) Which of the following elements are found free (elemental) in nature? P, Mg, K, S, Al, C, Br
5) Which family of elements is used in bulbs and lighted signs? Why?
6) What is special about the valence electrons (the ones that are involved in bonding) of the transition
metals?
7) What do the metals in the Actinide series have in common? What special property do iron, cobalt
and nickel share?
8) How is the design of the periodic table reflective of periodic law?
9) What is the impact of nuclear charge and shielding on atomic radius?
10) How does atomic radius influence electronegativity and ionization energy? What impact does that
have on reactivity of metals vs non-metals?
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Study Guide
Chemistry Test #5
Directions: Match the appropriate definition with each key term
1. Metal
a)
Form ions by gaining electrons
2. Electronegativity
b)
Group 17 elements
3. Atomic radius
c)
Horizontal rows in periodic table
4. Anion
d)
d-block elements
5. Alkali metals
e)
Elements that do not react
6. Ionization energy
f)
7. Non-metal
g)
Atom that has lost or gained electrons and become a
charged particle
Vertical columns in periodic table
8. Cation
h)
9. Halogens
i)
10. Valence electrons
j)
11. Periods
k)
Energy required to remove an electron from an
atom
Negatively charged ion
12. Groups
l)
The ability of an atom to attract an electron
13. Noble gases
m) Group 1 elements
14. Transition metal
n)
Electrons in the outermost energy level
15. ion
o)
Formed when atoms LOSE electrons
Elements that are conductors, are bendable and
have luster
The size of the atom
1) Which class of elements will LOSE electrons during bonding? Explain why based on ionization
energy and/or electronegativity.
2) Which class of elements will GAIN electrons during bonding? Explain why based on ionization energy
and/or electronegativity.
3) For each group in the s and p blocks, identify the number of valence electrons:
Group #
1
2
13
14
15
16
17
18
Valence e
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Study Guide
Chemistry Test #5
Trends-Atomic size, Shielding, Ionization Energy, Electron Affinity
1. Circle the one from each pair that would be the larger in size:
(A) F atom or O atom
(B) Ba atom or Ra atom
(C) Hf atom or Ti atom
(D) Cs ion or Ba ion
(E) Al ion or Al atom
(F) Po ion or At ion
2. Circle the element that has more shielding:
(A) B or In
(B) Mg or S or neither
(C) Tl or Y
(D) Cl or I
(E) Ar or Xe
(F) Ca or Ga or neither
3. Circle the element with the greater first ionization energy (IE):
(A) Pb or Sn
(B) B or C
(C) Ba or At
(D) Lr or Ra
(E) Cs or V
(F) Si or Ag
4. Circle the element with the greater electron affinity (EA):
(A) F or Cl
(B) Sr or Rb
(C) Os or Co
(D) Am or Eu
(E) Pb or Sn
(F) Ba or At
5. Circle the element with the lower electronegativity (EN):
(A) C or N
(B) Na or K
(C) Ta or Cu
(D) Pd or Mo
(D) Lr or Ra
(E) Cs or V
1) What is the difference between electron affinity and ionization energy?
2) Why does oxygen have a higher ionization energy than selenium?
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Study Guide
Chemistry Test #5
Use the periodic table below to answer the questions below it.
G
H
1) Between B and C, the highest electronegativity level?
2) Highest ionization energy
3) Between C and G, the largest atomic radius
4) Most reactive metal
5) Between B and E, the smallest atomic radius
6) Lowest electron affinity
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