Download Honors Chemistry- Chapter 5 Homework Packet The Periodic Law

Honors Chemistry- Chapter 5 Homework Packet
The Periodic Law and Periodic Properties
1) (a) How do the electron configurations within the same group of elements
compare?
(b) Why are the noble gases relatively unreactive?
2) What is the relationship between the electron configuration of an element and the
period in which that element appears on the periodic table?
3) (a) What information is provided by the specific block location of an element?
(b) Identify, by number and location, the four blocks of the periodic table.
4) (a) Which elements are designated at the alkali metals?
(b) List four of their characteristic properties.
5) (a) Which elements are designated as the alkaline-earth metals?
(b) How to their characteristics compare with those of the alkali metals?
6) Write the noble gas notation for each of the following elements and indicate in
which period each element belongs.
(a) Li
(b) O
(c) Br
(d) Sn
7) What is the name often used to refer to the entire set of d-block elements?
8) What types of elements make up the p-block? Where in the block is each type
generally located?
9) (a) Which elements are designated as halogens?
(b) List four of their characteristics.
10) What are the main-group elements?
11) Without looking at the periodic table, identify the period, block, group, type of
element, and relative reactivity for elements with the following electron
configurations.
(a) [Ne] 3s2
Period
Block
Group
Element type
Reactivity
(b) [Kr] 5s24d105p5
Period
Block
Group
Element type
Reactivity
(c) [Ar] 4s1
Period
Block
Group
Element type
Reactivity
(d) [Xe] 6s24f155d106p6
Period
Block
Group
Element type
Reactivity
12) (a) Where are valence electrons located?
(b) What is the importance of valence electrons?
13) Which elements are designated as the noble gases? What is their most
significant property?
14) How is the atomic radius of an element defined?
15) What trend is observed for atomic radius across a period? Provide an
explanation.
16) What trend is observed for atomic radius down a group? Provide an
explanation.
17) (a) What is a cation?
(b) What is an anion?
(c) What is the first ionization energy of an atom?
18) What trend is observed for first ionization energy across a period? Provide an
explanation.
19) What trend is observed for first ionization energy down a group? Provide an
explanation.
20) Complete the following table.
Group
Electrons lost or
gained in compound
formation?
# of electrons lost or
gained
Ion formed
1
2
13
15
16
17
18
21) How do the values of successive ionization energies within one atom compare?
Provide an explanation.
22) (a) Without looking at a table of ionization energies, arrange the following
elements in order of decreasing first ionization energy.
Li
O
C
K
Ne
F
(b) Now…. Which of the above elements would you expect to have the highest
second ionization energy and why?
23) (a) Which of the following cations is least likely to form?
Sr2+
Al3+
K2+
(b) Which of the following anions is least likely to form?
I-
S3-
O2-
24) The two ions K+ and Ca2+ each have 18 electrons surrounding the nucleus.
Which has a smaller radius and why?
25) (a) How does the size of a cation compare to its neutral atom? Provide an
explanation.
(b) How does the size of an anion compare to its neutral atom? Provide an
explanation.
26) Which of the following does NOT have a noble-gas configuration?
Na+
Rb+
O2-
Br-
Ca+
Al3+
S2-
27) For each element below, determine the charge of the ion that is most likely to be
formed.
Element
Ion Formed
Element
Li
P
Mg
O
Cs
Ba
F
Br
Al
N
Ion Formed
28) (a) What is electronegativity?
(b) Why is fluorine special in terms of electronegativity?
(c) In which corner of the periodic table do the elements have the highest
electronegativity? In which corner do they have the lowest electronegativity?