1. Physical Science
Ch. 20

2. Section 1
Metals

3. Properties of metals Conduct heat and electricity Luster Malleable
reflect light well
Malleable
can be hammered or rolled into sheets
Ductile
can be drawn into wires
Electron Donors
combine with nonmetals by losing electrons

4. Metallic Bonding
Positively charged metallic ions are surrounded by a cloud of electrons
Ions are in sliding layers and electrons are weakly held
Readily form ionic bonds with nonmetals

5. The Alkali Metals softer and more reactive than other metals
Highly reactive w/ oxygen & water
don’t occur naturally as elemental forms
Combine readily with other elements due to single electron in outer energy level
Located in 1st column of periodic table

6. Uses of Alkali Metals Human health Photocells Francium
sodium, potassium, and lithium compounds
Photocells
some depend on rubidium or cesium
Francium
a radioactive element which breaks down giving off particles and energy

7. The Alkaline Earth Metals
not found naturally in elemental form
two electrons in outer energy level
Located in the 2nd column of the periodic table

8. Alkaline Earth Metals The Applications Uses with the Human body
strontium and magnesium found in fireworks
magnesium in vehicles, ladders, and bats
calcium in statues and countertops
Uses with the Human body
calcium in bones
barium in disease diagnoses
radium formerly used in cancer treatments

9. Transition Elements They often occur in nature as uncombined elements
Located in the sunken in area of the periodic table
The number of valence electrons have a tendency to vary (transition) at times

10. Transition Elements Typically form colored compounds
chromium is in rubies & emeralds
Iron triad (iron, cobalt, and nickel)
Iron
most widely used of all metals
main ingredient in steel
abundant in Earth’s crust
Cobalt and nickel
used in some steels
Nickel
used to coat other metals

11. Copper, silver, gold Copper Silver Gold Zinc and cadmium Mercury
coinage metals since once were commonly used in coins
Copper
used in electric wiring because it is a superior electricity conductor
Silver
used in photographic film and paper; jewelry
Gold
used in jewelry
Zinc and cadmium
often used to coat or plate other metals
Mercury
only room temperature liquid metal
used in thermometers and batteries

12. Inner Transition Metals
Rare earth elements
seem disconnected from the rest of periodic table
The Lanthanides Series (1st row)
The Actinides (2nd row)
All are radioactive and unstable
Uranium is the best known

13. Section 2
Nonmetals

14. Nonmetals Properties of nonmetals
Gases or brittle solids at room temperature
Not malleable
Not ductile
Poor conductors of heat and electricity
Lustrous
Electron acceptos

15. Compounds formed by Nonmetals
Ionic compounds
form when nonmetals gain electrons from metals and become negative ions
Covalent compounds
form when nonmetals share electrons with other nonmetals

16. Sublimation Diatomic molecule
a solid changes directly into a gas without first becoming a liquid
Diatomic molecule
two atoms of the same element in covalent bond

17. Magnificent Seven Bromine Oxygen Fluoride Iodine Nitrogen Chlorine
7 diatomic elements
Always occur with 2 atoms
Bromine
Oxygen
Fluoride
Iodine
Nitrogen
Chlorine
Hydrogen

18. More about nonmetals Hydrogen most common element in universe
diatomic molecule
Highly reactive element found mostly on Earth as part of water compound

19. More about nonmetals The Halogens (7th column) Use of halogens
A salt forms when a halogen gains one electron from a metal
Use of halogens
Chlorine
disinfectant and bleach
Bromine
dyes in cosmetics
Iodine
hormone regulation

20. Noble Gases Exist as isolated, stable atoms Located in 8th column
Have complete outer energy level filled
Helium
used in blimps and balloons
Neon, argon, and krypton
used in lights

21. Section 3
Mixed Groups

22. Properties of metalloids
Located around the stair steps
Form ionic & covalent bonds
Have some metallic & some non-metallic properties
Partial conduction gives them semiconductor characteristics

23. Boron Group Named for the first element in 3rd column
Has 3 valence electrons
Boron
used in water softening products, antiseptics, and fuels
Aluminum
abundant in Earth’s crust
used in cans, foil wrap, pans, building materials, and aircraft

24. Carbon Group Named for first element in 4th column
Four valence electrons
Carbon
found in coal, oil, natural gas, and foods
Silicon
Occurs as an allotrope
same element with different molecular structures
Found in sand, rocks, and soil
The main component in semiconductors
conduct electricity under certain conditions

25. Carbon Group con’t Germanium Tin Lead Allotropes of carbon
also used in semiconductors
Tin
used to coat other metals
Lead
toxic, so no longer used in paint
Allotropes of carbon
Diamonds
Graphite
Buckminsterfullerene

26. Nitrogen Group Named for first element in 5th column
Has five valence electrons
tends to form covalent bonds
Nitrogen
used to make nitrates and ammonia
Phosphorus
used in water softeners, fertilizers, match heads, fine china
Antimony and bismuth
used with other metals to lower their melting points

27. Oxygen Group Named for first element in 6th column
Has six valence electrons
Oxygen
makes up 20% of air
is used by living things in respiration
provides protection from Sun’s radiation
Sulfur
used to form sulfides for pigment in paint
Selenium
used in photocopiers and multivitamins

28. Synthetic Elements (man made)
Created elements not usually found on Earth
synthetic elements usually disintegrate quickly.
Uranium
can be made into neptunium which forms plutonium when it disintegrates.
Plutonium
can be changed into americiun
used in smoke detectors.
Transuranium elements
have more than 92 protons
are synthetic and unstable

29. The study of synthesized elements helps scientists to understand the forces holding the nucleus together.
Element 114 lasted for 30 seconds.
It combined 114 protons with 175 neutrons.
It broke apart due to enormous repulsion between the protons.