Honors Chemistry
Name: _____________________________ Date: ______________
Mods: _______
Chapter 7:
Periodic Properties
Review Packet
7.1 - DEVELOPMENT OF THE PERIODIC TABLE
1) ______________ _________________ published the first classification scheme for the
elements by placing them in order of increasing ______________ ______________.
2) _____________ __________________ developed the concept of atomic numbers and
reorganized the periodic table in order of increasing atomic number.
3) Find an example in the periodic table where increasing atomic number does not match
increasing atomic weight.
7.2 - EFFECTIVE NUCLEAR CHARGE & ELECTRON SHIELDING
1) What two things does the force of attraction between an electron and the nucleus of an atom
depend on?
2) As you move across a period (leftright), effective nuclear charge _________________. This
is due to the fact that there are a greater number of _______________ in each atom as you
move across a period, but all of the electrons are in the same main __________ __________.
Therefore going across a period, the attraction between the nucleus and outer valence
electrons __________________.
3) As you move down a column and the value of n increases, the inner core electrons help to
________________ the outer (or valence) electrons from the attraction of the nucleus.
Therefore, there is a(n) _________________ in electron shielding as the _________________
___________________ number increases, resulting in electrons being ___________ attracted
to the nucleus.
4) Therefore, effective nuclear charge becomes the basis for all trends moving _____________
___ ______________, while electron shielding becomes the basis for all trends moving
_____________ ___ ______________.
7.3 - SIZES OF ATOMS & IONS
1) Define atomic radius-
2) The bonding atomic radius is ___________ in length than the non-bonding atomic radius.
3) Atomic radius generally ____________________ as you move across a period due to the
__________________ attraction between the atom’s nucleus and outer electrons (results from
the effective nuclear charge).
4) Atomic radius generally _______________________ as you move down a column due to the
__________________ attraction between the atom’s nucleus and outer electrons (results from
the shielding effect and increased n value)
5) Which element has the largest atomic radius? ________________________________
6) Rank each of the following sets of atoms from smallest to largest atomic radius.
a. C, Li, F
b. Na, Li, K
c. O, Ge, P
d. Si, C, N
7) Cations are _______________ than their parent atoms due to the ______________ of
electrons, but anions are _______________ than their parent atoms due to the
_______________ of electrons
8) Ionic size generally ______________________ as you move down a column (follows same
general trend as atomic radius)
9) Define isoelectronic series-
O2-, F-, Na+, Mg2+, and Al3+
10) Answer a-c below for the following isoelectronic series:
a) How many electrons does each ion in the series have? ____________
b) Which ion has the largest radius? ____________
c) Which ion has the smallest radius? _____________
7.4 - IONIZATION ENERGY
1) Define 1st ionization energy-
2) Ionization energy generally ____________________ as you move across a period, meaning
that a ________________ amount of energy is required to remove an electron. Again, this is
due to a(n) ____________________ attraction between the nucleus & outer electrons.
3) Ionization energy generally ____________________ as you move down a column because it
is _________________ to remove an electron which is further from (and ___________
attracted to) the nucleus.
4) Which element has the highest 1st ionization energy? ___________________________
5) Rank each of the following sets of atoms from lowest to highest 1st ionization energy.
a.
Mg, Si, S
b.
Mg, Ba, Ca
c.
Ne, Cu, Ba
d.
Si, P, N
6) Which family has the highest 2nd ionization energy? _____________________________
7) Which family has the highest 4th ionization energy? _____________________________
8) Show how the electron configuration changes from an atom of Fe to the Fe2+ ion.
Fe:
Fe2+:
9) Show how the electron configuration changes from an atom of P to the P3- ion.
P:
P3–:
7.5 - ELECTRON AFFINITY
1) Define electron affinity-
2) For most atoms, energy is __________________ when an electron is added, resulting in a
negative value for electron affinity in kJ/mol. Recall that atoms are more stable at
_____________ energy, meaning that a __________ of energy is more favorable for the atom.
3) Which family has all positive values for electron affinity and why do you think this is?
4) Which family has the highest negative values for electron affinity and why do you think this is?
PG. 312 - ELECTRONEGATIVITY
1) Define electronegativity-
2) Which family is not included in Pauling’s electronegativity scale? Explain why.
3) Which element has the highest electronegativity value? _______________________
4) Electronegativity generally ______________________ as you move across a period due to
a(n) ___________________ in effective nuclear charge.
5) Electronegativity generally ______________________ as you move down a column due to
a(n) ___________________ in electron shielding and principle quantum number. This results
in a ___________________ ability to attract electrons towards the atom and its nucleus.
6) Rank each of the following sets of atoms from lowest to highest electronegativity.
a.
N, C, Li
b.
Ne, O, C
c.
O, P, Si
d.
Mg, K, P
7.6 - METALS, NONMETALS, AND METALLOIDS
1) Metallic character generally _______________________ as you move across a period.
2) Metallic character generally _______________________ as you move down a column.
Chapter 7- Review & Practice Problems:
1. In each of the following sets (a-d), circle the element with the highest first ionization energy:
(a) Li, K, Cs
(b) S, Cl, Ar
(d) Cl , Na, Na+
(c) Br, I, Te
2. In each of the following sets (a-e), circle the element with the largest atomic/ionic radius:
(a) Sr, Rb, Ba
(b) O2-, S, S2-
3. Circle the best choice in each list:
(a) highest first ionization energy:
N, B, Li
(c) Cu, Ni, C
(d) K+, K
(e) P, N, As
(b) highest electronegativity: Te, Se, S
(c) smallest atom: K, Fr, Be
(d) highest (most negative) electron affinity: Se, Cl, Sb
(e) lowest first ionization energy: Ca, Ga, K
(f) highest second ionization energy: Na, Mg, Al
(g) lowest second ionization energy: Ar, K, Ca
4. Give an example of an isoelectronic series that contains 5 atoms or ions that each have
18 e– (Note: it is necessary to represent an ion by its symbol and charge.)
5. Fill in the table below to write the noble gas configurations for the following atoms and ions:
Atom
Atom’s
Noble Gas Configuration
Ion
formed
# of electrons
lost or gained
(must specify)
Ion’s
Noble Gas Configuration
Na
[Ne]3s1
Na+
1 e– lost
[He]2s22p6
(a)
S
S2–
(b)
Al
Al3+
(c)
Br
Br –
(d)
Mg
Mg+
(e)
N
N2–
(f)
Fe
Fe3+
6. Fill in the table below to practice with ions:
Element
Lithium
Charge
Ion
Symbol
Name of ion
Atom’s
electrons
Ion’s
electrons
Like which
noble gas?
+1
Li1+
lithium
3
2
Helium
55
54
Ba2+
(a)
(b)
Chlorine
(c)
(d)
-3
15
Gallium
(e)
N/A
O2-
(f)
7. Answer the following questions regarding periodic trends for these atoms:
(a) Which element has the highest first ionization energy?
____________
(b) Which element has the lowest electronegativity?
____________
(c) Which element has the most metallic character?
____________
(d) Which element is the smallest atomic radius?
____________
8. Answer the following questions regarding periodic trends for these atoms:
(a) Which element has the lowest first ionization energy?
____________
(b) Which element has the highest electron affinity?
____________
(c) Which element has the least metallic character?
____________
(d) Which element has the largest ionic radius?
____________
(e) Which element is most likely to gain 2 electrons?
____________
9. Answer the following questions regarding periodic trends for these atoms:
(a) Which element has the highest first ionization energy?
____________
(b) Which element has the highest electronegativity?
____________
(c) Which element has the most metallic character?
____________
(d) Which element has the largest atomic radius?
____________
(e) Which element has the greatest electron shielding?
____________
Li, Be, Mg, Na
P, S, Cl, F
Au, Zn, S, Si
10. In each set below, circle the smallest atom or ion and underline the largest atom or ion.
(a) H+, He
(b) K+, Ca2+, Ar, Cl–, S2–
(c) F–, Cl–, Ba2+, Sr2+