1. ELEMENTS: CHEMICAL & PHYSICAL PROPERTIES

2. GROUP 1 Alkali Metals Potassium reaction with water Sodium reaction
Are not found as elements in nature
Stored under kerosene or other hydrocarbon solvent (oil)
Can react with water vapor or oxygen in the air
Good conductors of electricity and heat
Ductile, malleable, and soft
Silvery luster
Low density
Low melting point
Form:
colorless ions with a 1+ charge
ionic compounds
water-soluble bases
Potassium reaction
with water
Sodium reaction
with air

3. GROUP 2 Alkaline Earth Metals
Are not found as elements in nature
Occur most commonly as carbonates, phosphates, silicates, and sulfates
Good conductors of electricity and heat
Ductile and malleable
Silvery luster
Includes naturally radioactive element radium
Form:
less reactive than alkali metals
rxn with HOH to form bases & hydrogen gas compounds are insoluble or only slightly soluble in water
forms primarily ionic compounds
ions with a 2+ charge
Beryl
A source of beryllium

4. GROUPS 3 – 12 Transition Metals
Usually harder, more brittle than Groups 1 & 2 metals
Higher melting & boiling points than Groups 1 & 2 metals
Good conductors of electricity and heat
Malleable and ductile
Silvery luster, except copper & gold
Chemical properties differ from each other
Include radioactive elements
Compounds often colored
May form complex ions
1 or 2 valence electrons
Usually have ≥ 2 common oxidation states
Includes mercury, only metal that is liquid at room temperature ↓
Transition
metals

5. GROUP 13 Boron Family are not found as elements in nature
scarce in nature
metallic solids
soft, low melting points
chemically reactive at moderate temperatures
3 valence electrons
Exceptions:
aluminum: most abundant metallic element which exists as
ore bauxite, is self-protecting
boron: metalloid, covalent solid, hard, high melting point,
not chemically reactive at moderate temperatures

6. GROUP 14 Carbon Family nonmetal: carbon metalloids: silicon, germanium
metals: tin, lead
large variation in physical & chemical properties
occurs in elemental & combined forms
relatively unreactive
4 valence electrons
tend to form covalent compounds although tin and lead will form ionic compounds
Tin and lead are self-protecting metals

7. GROUP 15 Nitrogen Family nonmetals: nitrogen, phosphorus
metalloids: arsenic, antimony
metal: bismuth
Most common forms:
nitrogen: atmospheric N2
phosphorus: phosphate rock
arsenic, antimony, bismuth: sulfides or oxides
antimony, bismuth: elements
abundant : nitrogen, phosphorus
rare: arsenic, antimony, bismuth
form covalent compounds, oxidation numbers usually +3 or +5
atoms have 5 electrons in their outermost energy level
Exist in ≥2 allotropic forms except nitrogen & bismuth
Solids at room temperature, except nitrogen

8. GROUP 16 Oxygen Family nonmetal: oxygen, sulfur, selenium
metalloid: tellurium
metal: polonium
occur as elements & in combined states
form covalent compounds, oxidation numbers usually -2
atoms have 6 electrons in outermost energy shell
often exist as diatomic & polyatomic molecules (i.e. O2, S6)
exist in several allotropic forms (i.e. sulfur can exist as orthorhombic or monoclinic crystal structure)

9. GROUP 17 Halogens all nonmetals
occur in combined form, usually as metal halides
found in rocks of Earth’s crust & dissolved in sea water
At room temperature --- gas: F Cl2
liquid: Br2
solid: I2
all reactive, esp. fluorine
Atoms have 7 electrons in outermost energy level
Usually gain an electron to form a halide, X- ion, but can share electrons & have positive oxidation states

10. GROUP 18 Noble Gases inert
essentially demonstrate ideal gas behavior over a wide range of temperatures & pressures
group has highest ionization energy, therefore strongly resist losing electrons
complete octet of electrons in highest energy level
gases at room temperature
1st noble gas compound prepared in 1962, XeF4
Neon, Argon, Krypton Xenon used in lighting
Helium used in balloons since less dense than air