SO₃^2-

Chlorite

Physical Changes

1. Changes that alter appearance of matter w/o altering composition.
2. State Changes:
   1. Boiling/condensing
   2. melting/freezing
   3. subliming of ice
3. Dissolving

Chemical Changes

1. Changes that alter the composition of matter.
2. Examples:
   1. Rusting
   2. releasing energy
   3. burning

Kinetic Energy

1. Energy of Motion (motion of atoms, molecules, and subatomic particles).
2. Thermal Heat is an example because it is caused by molecular motion.

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Ex: A weight falling off a rooftop has ___ energy.

Ex: a weight hanging off the edge of a rooftop has high ___ energy and is unstable.

Ex 2: a weight sitting on the road after dropping has low ___ energy and is very stable.

Law that states: The total amount of energy in a system remains the same.

Energy_{Before Reaction} = Energy_{After Reaction}

Conversion formula

F-->C

Conversion Formula:

C-->K

Conversion Formula:

C-->F

1. The value depends on the quantity of matter.

EX: mass, volume, length, and total charge.

1. Value independent of the quantity of matter.

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EX: temperature, color, hardness, melting point, boiling point, pressure, molecular weight, and density

1. In a chemical reaction, matter is neither created nor destroyed.

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Mass_before = Mass_after

1. Proust: "All samples of a given compound (regardless of their source or how they were prepared) have the same proportions of their constituent element."

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Ex: 2 mol of H₂O contain same 2:1 (H:O) ratio as 4 mol H₂O.

1. Positively charged particles
2. mass of 1 amu
3. in nucleus

#p=atomic number

1. noncharged particles
2. mass of 1 amu
3. in nucleus

#n = Atomic Mass - #p

1. Negatively charged particles
2. mass of about 0 amu
3. in empty space around nucleus

#e=#p (except in ions)

atomic number

the number of protons in the nucleus of an atom

⁵B

10.811

                 ^atomic mass

1. Atoms that have more neutrons than protons
2. Still behave similarly to neutral atom

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 Ex: Ne-21 (¹⁰Ne)

 #p: 10, #n=21-10=11

1. Charged particles (from the gain or loss of e-)
   1. gain: become anions (-)
   2. lose: become cations (+) 
2. Behave differently from the neutral atom

1. Boron (B)
2. Silicon (Si)
3. Germanium (Ge)
4. Arsenic (As)
5. Antimony (Sb)
6. Tellurium (Te)
7. Polonium (Po)

=∑(fractional abundance of isotope)_n • (mass of isotope)_n

1. (M) = the mass of one mole of atoms.
2. element's atomic mass in amu's.

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EX: M_He= 4.003g/mol

Subscripts for

Hydrates and Prefixes

(1-10)

1. mono-               
2. di-
3. tri-
4. tetra-
5. penta-
6. hexa-
7. hepta-
8. octa-
9. nona-
10. deca-

Simplest whole number ratio of the atoms of elements in a compound.

EX: C₂H₄-->CH₂

1. A common technique for analyzing compounds
2. Burn a known mass of a compound and weigh the amounts of product made for C, O, and H.

C-->CO₂

H-->H₂O

Find O by subtracting mass from Sample_initial

1. "living compounds"
2. contain carbon and hydrogen
   1. also sometimes contain O, N, S, or P
3. Easy to decompose; more difficult to make (can do this now in the lab)

1. "Nonliving Compounds"
2. Harder to decompose, so easy to synthesize.

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EX: CO₂ (No H)

EX2: NCl₅

1. Contain only Carbon and Hydrogen atoms.
2. Most fuels made of these.
3. Different names:
   1. alkanes: single bonds 
   2. alkenes: one or more C=C
   3. alkynes: CºC
   4. aromatic: C6 “benzene” ring

1. Noncarbon group on the molecule 
2. substitute a non-carbon group for H on a hydrocarbon chain.

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