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Chapter 5: The Periodic Table
Atomic Radius decreases
lonization Energy increases
Electron Affin ity i ncreases
Electronegativity increases
Atomic Radius increases
lonization Energy decreases
Electron Affin ity decreases
E lectronegativity decreases
SHORT ANSWER:
'J".
a.
Who came up with the first useable Periodic Table?
b.
How did he arrange the elements?
c.
Why was his arrangement so ingenious (give two reasons)?
i.
ii.
d.
His arrangement produced some anomalies. Give an example.
2.
How did Moseley arrange the elements?
3.
How did Moseley determine the atomic number? Explain in detail (hint: hieh speed electrons, Xrays, metals).
4.
How did Dobereiner arrange the elements? Explain.
5.
Why was Newlands ridiculed for this version of the Periodic Table?
6.
Name each of the following groups:
a.
b.
c.
d.
e.
f.
Group L4:
Group 2A:
Group 7A:
Group 34:
Group 44:
Group 5A:
7.
Where are the transition metals on the periodic table (what orbitals do these atoms fill)?
8.
List the elements in the Lanthanide series:
9.
List the elements in the Actinide series:
10. Elements of the same group have the same number of
electrons.
11. The chemical and physical properties of the elements are periodic functions of their
, Elements with similar properties occur at
1-2. Define atomic radius:
discovered most of the Noble gases.
L3.
t4.
a.
b.
Moving down a group, the atomic radius
Why?
15.
a.
b.
Moving left to right across a period, atomic radius
why?
16.
a.
b.
Metals tend to have
why?
ionization energies.
17.
a.
b.
Nonmetals tend to have
ionization energies.
Why?
18.
a.
b.
Noble gases have
ionization energies.
Why?
19.
a.
b.
Moving down a group, ionization energy
Why?
24.
a.
b.
Why?
a.
What is electron affinity?
b.
Which group(s) has the highest electron affinity (most negative number)?
Moving left to right across a period, ionization energy
21-.
c. Which group(s) have the lowest electron affinity (positive numbers)?
22. Define electronegativity.
23. What element has the highest electronegativity?
24. Where are metals located on the periodic tables?
25. List 3 characteristics of metals:
a.
b.
26. Where are nonmetals located on the periodic table?
27. List three characteristics of nonmetals:
a.
b.
c.
28. List the metalloids:
29. What properties do metalloids have?
30. An element undergoes several ionizations as follows:
First:
740
kJ
Second: 1450
kJ
Third:
7730
kJ
Fourth: 9500
kJ
a.
b.
How many valence electrons does the atom have?
What group does it belong to?
31. Moving left to right in period 6, the electrons enter which sublevels (see electron
configuration)?
MULTIPLE CHOICE:
L
The relationship in which the physical and chemical properties of elements show a periodic
pattern when elements are arranged by increasing atomic number is called
c. Mendeleev's law
a. the periodic law
d. Meyer's periodicity
b. the law of octaves
2.
Who classified the elements into triads?
a. Mendeleev
b. Moseley
3.
d. Dobereiner
The scientist who observed a pattern of properties that repeated every eight elements was
a. Mendeleev
b. Moseley
4.
c. Newlands
c. Newlands
d. Dobereiner
Mendeleev arranged the elements in the periodic table in order of increasing
a.
b.
number
mass number
atomic
c. ionization energy
d. atomic mass
5.
ln the periodic table, the periods are
a.
b.
6.
7.
8.
columns
horizontal rows
c. chemicalfamilies
vertical
d. blocks of elements
How many elements are in the first period of the periodic table?
a.7
b.2
c. 18
a.
b.
halogens
c. alkaline earth metals
alkali metals
d. noble gases
d. L09
The elements in Group 14 of the periodic table are called the
The elements in Group 2A of the periodic table are called the
a.
b.
c. alkaline earth metals
halogens
d. noble gases
alkalimetals
9. What are the elements in Group 7A of the periodic table called?
c. alkaline earth metals
a. halogens
d. noble gases
b. alkali metals
10. Those electrons that are largely responsible for an atom's chemical behavior are called
b. high energy electrons
a. core electrons
c. stable electrons
b. valence electrons
1L. The second period of the periodic table contains
c.s, p, and d-block elements
a. s-block elements
d. p block elements
b. s and p-block elements
L2. Asystematicvariationinthepropertiesof elementsgoingdownagrouporacrossaperiodis
called
a
a.
b.
c. periodic trend
blockcharacteristic
periodic law
d. triad configuration
1-3. When an atom loses an electron,
a.
b.
it
c. becomes smaller
collapses
becomes negatively
charged d. becomes larger
14. When an atom becomes a negative ion, it
c. becomes larger
a. loses protons
b.
remains the same size
d. becomes smaller
1-5. A positively charged ion is called a
a.
b.
cation
c. anion
gluon
d. quark
L6. A negatively charged ion is called
a.
b.
1-7.
a
cation
c. anion
down quark
d. quark
Thefirstelectron removed from an tin (Sn) atom is (see electron figuration)?
a. 3p
b. 4d
c. 5s
d. 5p