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HCO3-
Hydrogen carbonate/ bicarbonate
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HPO42-
hydrogen phosphate
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H2PO4-
dihydrogen phosphate
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HSO4-
hydrogen sulfate/ bisulfate
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metals loose electrons -->
cations
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nonmetals gain electrons -->
anions
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group 1A
- alkali metals
- Li, Na, K, Rb, Cs, Fr
- highly reactive with water
- used to dry solvents
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group 2A
- Alkali earth metals
- Be, Mg, Ca, Sr, Ba, Ra
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group 3A
- B, Al, Ga, In, Tl
- Ga= galium is liquid at body heat and solid at room temp, can handle with hands
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impurites in oxides of aluminum=
creates colors in gems
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group 4A
- C, Si, Ge, Sn, Pb
- burn any compound= black ash (carbon compound)
- carbon= different forms, hardest compounds used to cut $$
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Group 5A
- N, P, As, Sb, Bi
- reacts with water
- used to dry solvents when alkali metals can't be used with flammable solvents
- NH3= ammonia, base, very common
- P was isolated from urine in 1669
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group 6A
- oxygen group
- O, S, Se, Te, Po
- O, S, Se = very similar
- Te and Po = not similar to O, S, Se
- Sulfur not found by itself
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group 7a
- Halogens
- F, Cl, Br, I, At
- very reactive
- not monomatic: never found as one atom
- ex: Cl always found as Cl2
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group 8A
- noble gases
- He, Ne, Ar, Kr, Xe, Rn
- don't react in normal environment, at extremes yes
- put in tubes and ecite electrons= neon sign
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compounds
- combo 2 + elements definite ratios by mass
- character of ea. element lost when compound is formed
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molecules
smallest unit of compound keeps characteristics of compound
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elements that exist as molecules
graphite, diamond, buckyballs
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elements that exist as diatomic molecules
H2, N2, (O2, O3), F2, Cl2, Br2, I2
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elements that exist as polyatomic molecules
P4, S8
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ions
atoms/ groups of atoms with pos. or neg. charge
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Iron (II), Iron (III)
Fe2+, Fe3+
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Cobalt (II), Cobalt (III)
Co2+, Co3+
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Copper (I), Copper (II)
Cu+, Cu2+
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electrons control the size of the ....
atom
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once you loose an electron...
the size of the atom shrinks
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negatively charged element cannot bind to ...
another negatively charged element
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