4.  Left side of periodic table
(80%)
 Conduct heat and electricity
 Reflect light
 Solids at room temperature
(one exception)

5.  Malleable ► Ductile

6.  Upper-right
 Great variation in
properties
 Most gases, some
solids, one liquid at
room temperature

7.  Poor conductors of
heat/electricity
 Brittle

8.  Along stair-step line
 Behave like a metal in some conditions,
nonmetal in others

10.  Russian scientist
 Published first
USEFUL periodic table
 Did not know atomic
structure, so he
arranged atoms by
mass

11.  Spaces left for “missing”
elements
 Were later discovered

13.  When atoms are
arranged by atomic
number (or atomic
mass, in
Mendeleev’s case),
there is a periodic
repetition of physical
and chemical
properties

15.  Atomic Number - # of protons
 Atomic Mass/Weight – Weighted average of mass
numbers of all isotopes

19.  Group 1A (except for
hydrogen)
 Comes from arabic word
meaning “the ashes”
because wood ashes are
rich in sodium and
potassium
 EXTREMELY reactive

20.  Group 2A
 Silver-colored, soft,
and low density metals
 Very reactive

21.  From the Greek “salt-generating”
 Group 7A
 Elements end in “–ine”
 Only group which contains all three states of matter
 EXTREMELY reactive

22.  Group 8A
 Rarely take part in chemical reactions
 Extremely low boiling points; rarely exist as liquids
 Used in lighting and lasers

23.  “B” groups of Periodic Table
 All solid metals, except for Mercury
 Strong, dense (often silvery-blue) solids that
make colorful solutions
Co Cr Ni Cu Mn

24.  f-block of Periodic
Table
 Usually unstable
 Often radioactive

26. Textbook Section 6.3

27.  Atoms do not have
sharply-defined
borders…
 Therefore, atomic size
is measured by the
distance between two
nuclei (atomic radius
is ½ this distance)

28.  Across a period, each atom has one
additional proton
 Increased force attraction pulls electrons
closer to nucleus (lowering the atom’s size)

29. Atomic size is greatest at the LEFT and the
BOTTOM of the periodic table

30.  When atoms bond
together to form
compounds, they share
electrons unequally
 “ability of an atoms to
attract electrons when in a
compound”

31.  Electronegativity is the greatest at the RIGHT
and TOP of the periodic table
 Exceptions: Noble gases