Transcript Chapter 3 part 2

Families of Elements
Chemistry
Learning Objectives
• TLW use the Periodic Table to identify and
explain the properties of chemical families
(TEKS 6.B)
• TLW color code the periodic table we’ve
been customizing
Agenda
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Ready, Set, Color Your Periodic Table
How Elements are Classified
Types of Metals
Types of Non-Metals
Review questions
Independent Practice – Periodic Table Puzzle
I. How elements are classified
A. Elements are classified as metals or
non-metals
1. Metals – elements that are good
conductors of heat and electricity;
a. Usually shiny solids;
b. Can be (can be shaped and hammered)
c. 88 elements are metal
d. Metals have 1, 2, 3, or 4 valence electrons
e. Metals tend to lose electrons in a chemical
reaction
ex. Rusting = iron will lose its valence
electrons
2. Non-metals – elements that are
poor conductors of heat and
electricity
a. Found on the right side of
periodic table
b. Non-metals can be solid, liquid,
or gas
c. Solid non-metals are very
brittle and dull
d. Non-metals gain electrons in a
chemical reaction
e. Non-metals have 5, 6, 7 or 8
valence electrons
3. Metalloids
a. elements that have properties
of both metals and nonmetals
b. they can conduct electricity
and heat, just not very well
B. Types of Metals
1. Alkali Metals
a. All alkali metals are found in
Group 1 (Column 1)
b. the alkali metals include: Li, Na,
K, Rb, Cs and Fr
c. Alkali metals are soft and shiny
d. All alkali metals react very
violently with H2O
Group No.
Noble Gases (brown)
Non-metals (green)
Halogens (orange)
Alkali Metals (blue)
Other metals
Alkaline Earth Metals (red) (turquoise)
2
13
Transition Metals (yellow)
Group
#
C
C
C
C
C
C
C
C
3
4
5
6
7
8
9
10
C
14 15 16
Cl
C
11 12
F
17
Ge
Br
I
Sb
Po
At
Metalloids (fushia)
Rare Earth
Metals
(gold)
e. all alkalis have 1 valence
electron; that is why they
are so reactive
f. Forms positive ions = lose
electrons (oxidation no. 1+)
g. alkali metals are only found in
nature as compounds, not
pure elements
2. Alkaline-earth Metals
a. Earth metals are in Group 2
b. Earth metals have 2 valence
electrons
c. Alkaline-Earth metals include: Be,
Mg, Ca, Sr, Ba, Ra
d. Forms positive ions = lose
electrons (oxidation no. 2+)
e. Ex. Of useful alkaline-earth metal
– milk of magnesia
Group No.
Noble Gases (brown)
Non-metals (green)
Halogens (orange)
Alkali Metals (blue)
Other metals
Alkaline Earth Metals (red) (turquoise)
2
13
Transition Metals (yellow)
Group
#
C
C
C
C
C
C
C
C
3
4
5
6
7
8
9
10
C
14 15 16
Cl
C
11 12
F
17
Ge
Br
I
Sb
Po
At
Metalloids (fushia)
Rare Earth
Metals
(gold)
3. Transition Metals
a. Found in the middle of the periodic table
b. In Groups 3-12
c. Not as reactive as Groups 1 and 2
d. Can be found in nature in pure form
e. Since easily shaped; many
transitional metals are used for
jewelry, wiring and others
f. Includes rare earth metals & radioactives
f. All transition metals lose electrons =>
so they form positive ions
(variable number of valence e- 1 to 4)
(oxidation numbers from 1+ - 4+)
g. Includes 68 elements
h. Some examples of transitional
metals include: Cu, Fe, Au, Ag,
Hg, Zn, etc
Group No.
Noble Gases (brown)
Non-metals (green)
Halogens (orange)
Alkali Metals (blue)
Other metals
Alkaline Earth Metals (red) (turquoise)
2
13
Transition Metals (yellow)
Group
#
C
C
C
C
C
C
C
C
3
4
5
6
7
8
9
10
C
14 15 16
Cl
C
11 12
F
17
Ge
Br
I
Sb
Po
At
Metalloids (fushia)
Rare Earth
Metals
(gold)
4. Other Metals
a. Part, but not all elements of Groups 13-16
b. form positive ions = loses electrons (oxidation
numbers usually 3+ or 4+)
c. includes: Al, Sn, Pb and others
d. some are called metalloids (metals/non-metal
properties)
Alloys
Alloys are materials that contain more than one metal
element and still maintain the characteristic properties of
metals
Alloys can be easier to work with, more durable, hold their
shape better, more corrosion resistant than any of the
pure metals they contain
Examples – steel (iron, chromium, nickel, and carbon),
brass (copper and zinc) and solder (lead and tin)
Group No.
Noble Gases (brown)
Non-metals (green)
Halogens (orange)
Alkali Metals (blue)
Other metals
Alkaline Earth Metals (red) (turquoise)
2
13
Transition Metals (yellow)
Group
#
C
C
C
C
C
C
C
C
3
4
5
6
7
8
9
10
C
14 15 16
Cl
C
11 12
F
17
Ge
Br
I
Sb
Po
At
Metalloids (fushia)
Rare Earth
Metals
(gold)
C. Non-metals
Groups – 13 - 18
1. Basic Non-Metals
a. Group 13 – 16 and H
b. Not reactive
c. Include: C, N, S, O, Si, P
d. Are gases or solids
e. Semiconductors – elements that can
conduct electricity, but aren’t metals
includes: B, Si, Ge, As, Sb, Te
C. Types of Non-metals
1. Basic Non-Metals
e. Groups 13 & 14 have 3 and 4 valence electrons,
respectively.
- Tend to lose electrons and become
positive. (oxidation numbers 3+ and 4+,
respectively)
f. Groups 15 & 16 have 5 & 6 valence electrons,
respectively. Tend to gain valence
electrons. Oxidation numbers are 3- and 2-,
respectively.
C. Types of Non-metals
2. Halogens
a. Highly reactive elements
b. Group 17
c. Halogens include: F, Cl, Br, I, At
d. Are gases in nature…
except Bromine which is a liquid
e. Notice they all end in “ine”
f. halogens gain electrons = forms
negative ions (oxidation number 1-)
Group No.
Noble Gases (brown)
Non-metals (green)
Halogens (orange)
Alkali Metals (blue)
Other metals
Alkaline Earth Metals (red) (turquoise)
2
13
Transition Metals (yellow)
Group
#
C
C
C
C
C
C
C
C
3
4
5
6
7
8
9
10
C
14 15 16
Cl
C
11 12
F
17
Ge
Br
I
Sb
Po
At
Metalloids (fushia)
Rare Earth
Metals
(gold)
3. Noble Gases
a. Elements in Group 18
b. Located on the far right side of the
periodic table
c. Nobel gases are the most non-reactive
elements
d. All noble elements are gases
e. Noble gases include: He, Ne, Ar, Kr, Xe, and Rn
Group No.
Noble Gases (brown)
Non-metals (green)
Halogens (orange)
Alkali Metals (blue)
Other metals
Alkaline Earth Metals (red) (turquoise)
2
13
Transition Metals (yellow)
Group
#
C
C
C
C
C
C
C
C
3
4
5
6
7
8
9
10
C
14 15 16
Cl
C
11 12
F
17
Ge
Br
I
Sb
Po
At
Metalloids (fushia)
Rare Earth
Metals
(gold)
f. All noble gases have 8 valence
electrons (except He with 2)
g. Since outer valence shell is filled, they
don’t react with other elements (oxidation
number is 0)
h. Because noble gases are nonreactive
they are called “inert” gases
i. Noble gases are mostly found as pure
elements, not in compounds
Group No.
Noble Gases (brown)
Non-metals (green)
Halogens (orange)
Alkali Metals (blue)
Other metals
Alkaline Earth Metals (red) (turquoise)
2
13
Transition Metals (yellow)
Group
#
C
C
C
C
C
C
C
C
3
4
5
6
7
8
9
10
C
14 15 16
Cl
C
11 12
F
17
Ge
Br
I
Sb
Po
At
Metalloids (fushia)
Rare Earth
Metals
(gold)
Section Questions
1. A shiny luster, can conduct
electricity, is malleable and is a
solid describes what?
metals
2. Cannot conduct electricity, and is
dull in luster describes what?
nonmetals
3. How many valence electrons do
metals have?
1, 2, 3, or 4
4. How many valence electrons do
nonmetals have?
5, 6, 7, or 8
5. If an element has properties of
both metals and nonmetals, it is
called a what?
metalloid
6. What kind of ions do metals form?
positive
7. What kind of ions do nonmetals
form?
negative
8. Where are the most reactive metals
found on the periodic table?
Left side – Group 1 – Alkali Metals
9. Where are the most stable, nonreactive
elements found on the periodic table?
Right side – Group 18 – Noble Gases
10. What are the elements in Group 17
called?
halogens
Independent Practice
• Periodic Table Puzzle