Download AKS Review

Name: _____ KEY _________
Date: __________
Pd.: ______
AKS Review: The Periodic Table
11) use the organization of the periodic table of elements to predict the properties of elements (GPS, HSGT)
(SCCH_B2005-11)
11a) use the periodic table to predict periodic trends including atomic radii, ionic radii, ionization energy,
electronegativity, reactivity, and oxidation number of various elements (GPS)
11b) compare and contrast trends in the chemical and physical properties of elements based on their position
on the periodic table (GPS)
11b1) identify metals, nonmetals, and metalloids
11b2) determine phases at room temperature
__________________________________________________________________________
1. Define the following terms:
Period- horizontal row on periodic table, repeating pattern of properties
Groups(families)- vertical column on periodic table. Elements in the same family have similar
properties because they have the same valence electron configuration
Periodic law- “Properties of elements are a Periodic Function of the atomic number.” When elements
are arranged by increasing atomic number there is a periodic repetition of chemical and physical
properties.
Periodic trend- The properties, atomic radius, ionization energy and electronegativity exhibit a pattern
(trend) horizontally across periods and vertically up or down groups.
Synthetic- Man Made, usually referring to elements that do not occur naturally
Ion- an atom or group of atoms having a charge due to excess or lack of electrons
a. Cation- particle having a positive charge (atoms lose electrons to become cations)
b. Anion- a particle having a negative charge (atoms gain electrons to become anions)
Electronegativity- tendency of an atom to hold electrons of other atoms in a bond; an arbitrary scale
indicating how tightly atoms hold electrons.
Ionization energy- Energy required to remove the most loosely held (outer) electron (first ionization
energy)
2. What were the contributions to the development of the Periodic Table of Mendeleev and Moseley?
Mendeleev arranged the periodic table by increasing atomic mass. He predicted that elements
like Ge would be discovered and what their properties would be. Using X-ray crystallography,
Moseley figured out that the periodic table should be arranged by increasing atomic number
instead of atomic mass.
3. Represent the valence electrons by
drawing Lewis diagrams for each element
across the second period.
4. Label the periodic table below as
follows:
a. Draw the location of the
staircase line
b. Shade the metal section, place
lines in the nonmetal section and
leave the metalloid section blank
c. Number Groups 1A-8A
d. Label the alkali metals, the
alkaline earth metals, the
transition metals, the halogens,
the noble gasses, the lanthanide
and actinide series.
IA = alkali metals
IIA = alkaline earth elements
All the B columns = transition metals
IIIA = boron family
IVA = carbon family
VA = nitrogen family
VI A = oxygen family
VII A = halogen family
VIII a = noble gases
5. What state are most elements in at room temperature? __
6. What two elements are liquid at room temperature? __
solid __
Hg, Br __
7. List several physical and chemical characteristics of:
Metals
Nonmetals
Metalloids
Physical
Malleable, ductile, luster
Conduct heat and electricity
Solids are brittle crystals
Poor conductors of heat and
electricity
Properties of both metals
and nonmetals.
semiconductors
Chemical
Corrode (with notable
exceptions)
Wide variety of properties
Properties of metals and
nonmetals
Lose electrons to form
positive ions (cations)
Phase (state of
matter)
All but Hg solid at room temp.
Gain electrons to form
negative ions (anions)
Various states at room temp.
All phases; solid, liquid, gas,
are represented
8. Fill in the trend and briefly explain why it occurs.
Trend
Atomic Radius
Ionization Energy
Electronegativity
Solids at room temp
Ionic radius
Group
Period
Increases down
because of added
energy levels
Increases to left because
of increased nuclear
charge to right
Increases up family
because valence
electrons of smaller
atoms are closer to
nucleus (held more
tightly).
Same as EI
Smaller atoms hold
electrons more tightly
than larger atoms
Increases to right
because larger atoms
lose electrons more
easily than smaller
(atomic radius)
Same as ionization
energy
Smaller atoms hold
electrons more tightly
than larger atoms
- Metal ions are
smaller than metal
atoms (lose valence
electrons)
- Nonmetal ions are
larger than nonmetal
atoms (gain valence
electrons)
Compare metal and
non metal
9. Describe the trend for reactivity in metals. Describe the trend for chemical activity (reactivity) in nonmetals.
Since metals lose electrons to react, larger metal atoms are more reactive than smaller ones. Metal
reactivity increases to left across a period (from staircase) and down a family. Francium is the most active
metal. Since nonmetals gain electrons to react, smaller nonmetal atoms are more reactive than larger
ones. Nonmetal reactivity increases to right across a period and up a family. Fluorine is the most active
nonmetal.
10. Which metal is most reactive? ___ Francium __
11. Which nonmetal is most reactive? _ Fluorine __
12. From the following series choose the element with the larger atomic radius between the two that are given
for each problem:
a. Na or Cs
b. K or Br
c. B or F
d. O or Se
13. From the following series choose the element with the smaller radius between the two that are given for
each problem:
a. Mg or Cl
b. K or K+
c. Cl or Cld. Ca+ or Br14. From the following series choose the element that is more electronegative and have a higher ionization
between the two that are given for each problem:
a. Fr or F
b. Li or Rb
c. Al or S
d. N or P
Use the list below to answer questions below
a. K
b. Ag
c. O
d. F
e. S
f. Kr
15. Which two elements have similar properties and why? _ P and S because they are in the same family and
have similar electron configurations _
16. Which element(s) is/are halogen(s)? _ F in column VIIA __
17. Which element(s) is/are transition metal(s)? _ Ag _
18. Which element(s) would form an anion? _ F, O, and S __
19. Which element(s) has/have a complete octet and is therefore unreactive? _ Kr _
20. Which element(s) has/have an oxidation number of -2? _ O and S _
21. Which Group(s) end(s) with ”s” sublevels? _ alkali metals & Alkaline earth metals _
22. Why is the d-block ten elements in width? There are 5 orbitals in the d-block. Each orbital holds a
maximum of two electrons.
23. What is the purpose of the staircase line? The line separates the metals and nonmetals, and shows
the location of metalloids.
24. How do metals become cations?
How do nonmetals become anions?
Metals lose electrons (negative particles) and become positively charged. Nonmetals gain
electrons and become negatively charged.
25. Use the graph below to answer the questions that follow.
TREND-ATOMIC RADIUS
ATOMIC RADIUS
2.5
2
1.5
1
0.5
0
3 4 5 C6 N7 O8 F9 Ne
10 Na
11Mg
12 Al
13 Si
14 15
16 17 18 19 20
P S Cl Ar K Ca
Li Be B C N O Fl Ne Na Mg Al Si P S Cl Ar K Ca
ATOMIC NUMBER-ELEMENTS
Atomic number
Li Be B
a. Which general trend exists for atomic size across a period? __ increases to left _
b. What general trend exists for atomic size down a family? ____ increases down the family _
c.
Which group has the largest size? __ alkali metals (1) __
The smallest? _ halogens (15) _
d. Why does atomic size decrease as you move left to right across a period? Nuclear charge increases
to the right across a period. Thus the electrons are pulled closer to the nucleus making the
atom smaller.
26. Why does atomic size increase as you move down a family/group? Moving down a family/group adds
energy levels full of electrons thus increasing the size of the atom.
27. Write the full electron configuration and short hand configuration for:
a. N
b. Sr
c. Cu
a. N [He] 2s2 2p3
b. Sr [Kr] 5s2
c. Sr [Ar] 4s2 3d9
1s2 2s2 2p3
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
1s2 2s2 2p6 3s2 3p6 4s2 3d9
28. Draw orbital diagrams for:
Ni and
Na