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

• 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

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

Group #C C C C C C C C C C

F

Cl

BrI

At

Non-metals (green)

Alkali Metals (blue)

Alkaline Earth Metals (red)

Group No.

Transition Metals (yellow)

Noble Gases (brown)

Halogens (orange)

Ge

Sb

Po

Other metals (turquoise)

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

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

Group #C C C C C C C C C C

F

Cl

BrI

At

Non-metals (green)

Alkali Metals (blue)

Alkaline Earth Metals (red)

Group No.

Transition Metals (yellow)

Noble Gases (brown)

Halogens (orange)

Ge

Sb

Po

Other metals (turquoise)

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

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

Group #C C C C C C C C C C

F

Cl

BrI

At

Non-metals (green)

Alkali Metals (blue)

Alkaline Earth Metals (red)

Group No.

Transition Metals (yellow)

Noble Gases (brown)

Halogens (orange)

Ge

Sb

Po

Other metals (turquoise)

Metalloids (fushia)

Rare Earth Metals (gold)

4. Other Metalsa. 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)

AlloysAlloys 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)

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

Group #C C C C C C C C C C

F

Cl

BrI

At

Non-metals (green)

Alkali Metals (blue)

Alkaline Earth Metals (red)

Group No.

Transition Metals (yellow)

Noble Gases (brown)

Halogens (orange)

Ge

Sb

Po

Other metals (turquoise)

Metalloids (fushia)

Rare Earth Metals (gold)

C. Non-metalsGroups – 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 solidse. Semiconductors – elements that can

conduct electricity, but aren’t metalsincludes: B, Si, Ge, As, Sb, Te

C. Types of Non-metals1. 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. Halogensa. 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-)

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

Group #C C C C C C C C C C

F

Cl

BrI

At

Non-metals (green)

Alkali Metals (blue)

Alkaline Earth Metals (red)

Group No.

Transition Metals (yellow)

Noble Gases (brown)

Halogens (orange)

Ge

Sb

Po

Other metals (turquoise)

Metalloids (fushia)

Rare Earth Metals (gold)

3. Noble Gasesa. 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

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

Group #C C C C C C C C C C

F

Cl

BrI

At

Non-metals (green)

Alkali Metals (blue)

Alkaline Earth Metals (red)

Group No.

Transition Metals (yellow)

Noble Gases (brown)

Halogens (orange)

Ge

Sb

Po

Other metals (turquoise)

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

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

Group #C C C C C C C C C C

F

Cl

BrI

At

Non-metals (green)

Alkali Metals (blue)

Alkaline Earth Metals (red)

Group No.

Transition Metals (yellow)

Noble Gases (brown)

Halogens (orange)

Ge

Sb

Po

Other metals (turquoise)

Metalloids (fushia)

Rare Earth Metals (gold)

Section Questions1. 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