2.  Have a ns 1 configuration  Form + 1 cations  Have only 1 valence electron  Reactivity increases down the column; reacts violently with H 2 O.  Forms basic compounds alkali. mp4

3.  Have a ns 2 configuration  Form + 2 cations  Have 2 valence electrons  Reactivity increases down the column; reacts violently with oxygen rather than H 2 O, but not as reactive as group 1.  Forms basic compounds (alkaline means “base”)

4.  Have a ns 2 (n-1)d (1-10) configuration  Cation charges transition (or change)  Fairly unreactive ; Fe reacts the most (especially with oxygen), while Au reacts the least  Form complex compounds and act as reaction catalysts vanadium.mp4

5.  Have a np 1 configuration  Form + 3 cations  Have 3 valence electrons  Mostly form covalent compounds  Boron is used to make glass; aluminum has never been found pure in nature – easily makes bonds

6.  Have a np 2 configuration  Form + 4 cations or - 4 anions  Have 4 valence electrons  Silicon is the most abundant compound on Earth  Carbon-carbon bonding is basis of organic chemistry and life

7.  Have a np 3 configuration  Form - 3 anions  Have 5 valence electrons  Mostly form covalent compounds  Form basic and acidic compounds

8.  Have a np 4 configuration  Form - 2 anions  Has 6 valence electrons  Reactivity varies; some are gases, others are metalloids; some form weak acids  Mostly found in minerals and the majority were discovered by accident!

9.  Have a np 5 configuration  Form - 1 anions  Have 7 valence electrons  Highly reactive with alkali and alkali earth metals; form acidic compounds  Nonmetals; mostly gases

10.  Always end with a np 6 configuration  Stable; don’t easily form ions  Have 8 valence electrons (no room for bonds)  Hardly reactive; known as the “inert” gases  With enough energy provided, can form compounds with halogens and chalcogens

11.  Have f orbital configurations  Lanthanides are used as catalysts in petroleum production; used in lamps, lasers, and magnets; often silvery-white soft metals that burn easily in air;  Actinides are radioactive; often release H 2 gas in reactions; are dense metals