Reactions

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CaS + H2O + CO2 -> Ca(HCO3)2 + H2S

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P + O₂--> P₂O₅

4P + 5O₂--> 2P₂O₅

The law of conservation of mass states, if you started out with 4 grams of Iron and 3 grams of Oxygen in the REACTANT, when they combine in the PRODUCT you would have a total of _____ grams of Iron oxide.

7

solution

A liquid that is a homogeneous mixture of two or more substances.

Synthesis

A+B= AB

Decompostion

AB= A+B

Law of Conservation of Mass

All chemical equations must be balanced. This means that the same number of atoms of each element must be found in both the reactants and the products of the reaction. Which scientific law does this illustrate?

Atomic Mass

The average of the masses of all the isotopes in an element

spectator ion

an ion that does not directly take part in a chemical reaction (appears unchanged on both sides)

C₈H₁₈ + O₂--> IO₂+ H₂O

can't work (law of converstion: matter and energy can never be changed or distroyed)

product

the "ending substance(s) in a chemical reaction

K3AsO4 + H2S -> As2S5 + KOH + H2O

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K3[Fe(SCN)6] + Na2Cr2O7 + H2SO4 -> Fe(NO3)3 + Cr2(SO4)3 + CO2 + H2O + Na2SO4 + KNO3

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K4Fe(CN)6 + KMnO4 + H2SO4 -> KHSO4 + Fe2(SO4)3 + MnSO4 + HNO3 + CO2 + H2O

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K4[Fe(SCN)6] + K2Cr2O7 + H2SO4 -> Fe2(SO4)3 + Cr2(SO4)3 + CO2 + H2O + K2SO4 + KNO3

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KBr + Al(ClO4)3 -> AlBr3 + KClO4

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KClO3 -> KCl + O2

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KClO3 -> KClO4 + KCl

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PbCrO₄ + HNO₃ → Pb(NO₃)₂ + H₂CrO₄

1 PbCrO₄ + 2 HNO₃ → 1 Pb(NO₃)₂ + 1 H₂CrO₄

S + N₂O → SO₂ + N₂

1 S + 2 N₂O → 1 SO₂ + 2 N₂

SO₂ + H₂O → H₂SO₃

1 SO₂ + 1 H₂O → 1 H₂SO₃

SO₃ + H₂O → H₂SO₄

1 SO₃ + 1 H₂O → 1 H₂SO₄

SiC + Cl₂ → SiCl₄ + C

1 SiC + 2 Cl₂ → 1 SiCl₄ + 1 C

composition reactions (general form)

A + B → AB

All chemical reactions are accompanied by, or involves a change in ___________.

energy

covalent bond

sharing of electrons

products

the resulting molecules or compounds in a chemical reaction. (what comes out)

(NH4)2BeF4 -> BeF2 + NH3 + HF

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(NH4)2Cr2O7 -> NH3 + H2O + Cr2O3 + O2

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(NH4)3AsS4 + HCl -> As2S5 + H2S + NH4Cl

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Ag2S + KCN -> KAg(CN)2 + K2S

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AgNO3 + FeCl3 -> Fe(NO3)3 + AgCl

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Al + FeO -> Al2O3 + Fe

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Al + HCl -> AlCl3 + H2

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Al + KOH + H2O -> KAlO2 + H2

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Al + NH4ClO4 -> Al2O3 + AlCl3 + NO + H2O

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Al + NaOH + H2O -> NaAl(OH)4 + H2

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Al + O2 -> Al2O3

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Al(NO3)3 + Na2CO3 -> Al2(CO3)3 + NaNO3

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BaCl2 + Al2(SO4)3 -> BaSO4 + AlCl3

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Be(OH)2 + NH4HF2 -> (NH4)2BeF4 + H2O

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Bi(NO3)3 + H2S -> Bi2S3 + HNO3

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C + SiO2 + Cl2 -> SiCl4 + CO

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C10H16 + Cl2 -> C + HCl

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C2H2 + O2 -> CO2 + H2O

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C2H3Cl + O2 -> CO2 + H2O + HCl

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C2H5OH + O2 -> CO + H2O

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C2H5OH + O2 -> CO2 + H2O

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C3H8 + O2 -> CO2 + H2O

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C4H10 + O2 -> CO2 + H2O

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C6H6 + O2 -> CO2 + H2O

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Ca3(PO4)2 + SiO2 + C -> CaSiO3 + P4 + CO

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Ca3(PO4)2 + SiO2 -> CaSiO3 + P2O5

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Ca3(PO4)2 + SiO2 -> P4O10 + CaSiO3

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Ca3P2 + H2O -> Ca(OH)2 + PH3

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Ca5F(PO4)3 + H2SO4 -> Ca(H2PO4)2 + CaSO4 + HF

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CaCN2 + H2O -> CaCO3 + NH3

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CaHPO4⋅2H2O + NaOH + H2O -> Na2HPO4⋅12H2O + Ca(OH)2

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CaS + H2O -> Ca(HS)2 + Ca(OH)2

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CaS2 + O2 -> CaS2O3

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Cr(OH)3 + H2SO4 -> Cr2(SO4)3 + H2O

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FeCl3 + Ca(OH)2 -> CaCl2 + Fe(OH)3

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FeCl3 + NH4OH -> Fe(OH)3 + NH4Cl

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FeO + H3PO4 -> Fe3(PO4)2 + H2O

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FeS + O2 -> Fe2O3 + SO2

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FeS2 + O2 -> Fe2O3 + SO2

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FeSO4 + K3[Fe(CN)6] -> Fe3[Fe(CN)6]2 + K2SO4

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H2S + Cl2 -> S8 + HCl

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H2SO4 + Al(OH)3 -> Al2(SO4)3 + H2O

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H2SO4 + HI -> H2S + I2 + H2O

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H2SO4 + NaHCO3 -> Na2SO4 + CO2 + H2O

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I2 + HNO3 -> HIO3 + NO2 + H2

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K2CO3 + C + N2 -> KCN + CO

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K2MnO4 + H2SO4 -> KMnO4 + MnO2 + K2SO4 + H2O

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KNO3 + C12H22O11 -> N2 + CO2 + H2O + K2CO3

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KO2 + CO2 -> K2CO3 + O2

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KOH + AlCl3 -> KCl + Al(OH)3

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Mg3N2 + H2O -> Mg(OH)2 + NH3

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MgNH4AsO4 + 6H2O -> Mg2As2O7 + NH3 + H2O

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MgNH4PO4 -> Mg2P2O7 + NH3 + H2O

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MnO2 + HCl -> MnCl2 + H2O + Cl2

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Na3AsO3 + H2S -> As2S3 + NaOH

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NaCl + H2SO4 -> Na2SO4 + HCl

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NaOH + Cl2 -> NaCl + NaClO + H2O

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NaOH + Zn(NO3)2 -> NaNO3 + Zn(OH)2

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NiS + O2 -> NiO + SO2

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P4 + H2O -> H3PO4 + H2

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P4 + O2 -> P2O5

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P4O10 + H2O -> H3PO4

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P4O10 + HCl -> POCl3 + HPO3

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P4O6 + H2O -> H3PO3

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P4O6 -> P4 + P2O4

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PCl3 + H2O -> H3PO3 + HCl

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Si + NaOH + H2O -> Na2SiO3 + H2

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Si + S8 -> Si2S4

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Si2H3 + O2 -> SiO2 + H2O

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SiCl4 + H2O -> H4SiO4 + HCl

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SiH4 + O2 -> SiO2 + H2O

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SiO2 + HF -> SiF4 + H2O

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Sn(OH)2 + NaOH -> Na2SnO2 + H2O

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Sn(OH)4 + NaOH -> Na2SnO3 + H2O

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TiCl4 + Mg -> MgCl2 + Ti

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(CuOH)₂CO₃ → CuO + CO₂ + H₂O

1 (CuOH)₂CO₃ → 2 CuO + 1 CO₂ + 1 H₂O

CaCO₃ + HCl → CaCl₂ + H₂O + CO₂

1 CaCO₃ + 2 HCl → 1 CaCl₂ + 1 H₂O + 1 CO₂

CaC₂ + N₂ → CaCN₂ + C

1 CaC₂ + 1 N₂ → 1 CaCN₂ + 1 C

NaCl + NH₄HCO₃ → NaHCO₃ + NH₄Cl

1 NaCl + 1 NH₄HCO₃ → 1 NaHCO₃ + 1 NH₄Cl

NaPO₃ + CuO → NaCuPO₄

1 NaPO₃ + 1 CuO → 1 NaCuPO₄

CO + O₂ → CO₂

2 CO + 1 O₂ → 2 CO₂

ClO₂ + H₂O → HClO₂ + HClO₃

2 ClO₂ + 1 H₂O → 1 HClO₂ + 1 HClO₃

NaOH + FeSO₄ → Na₂SO₄ + Fe(OH)₂

2 NaOH + 1 FeSO₄ → 1 Na₂SO₄ + 1 Fe(OH)₂

chemical reaction

A _____ _____ when substances interact to form one or more new substances with different properties than the original substances.

Anion

A negative ion

double replacement reactions (general form)

AB + CD → AD + CB

Isotopes

Atoms of the same element that have different numbers of neutrons

1

Barium atoms = ________

8

How many Boron?

18

Oxygen atoms = ________

6

Silicon atoms = ________

aqueous substance

that substance is dissolved in water

Aluminum oxide

this is the way to write the chemical formula

element symbol above an →

used to indicate a catalyst

(NH4)2Cr2O7 -> Cr2O3 + N2 + H2O

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Al(OH)3 + H2SO4 -> Al2(SO4)3 + H2O

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Al2(SO4)3 + Ca(OH)2 -> CaSO4 + Al(OH)3

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Al2O3 + C + N2 -> AlN + CO

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Al4C3 + H2O -> CH4 + Al(OH)3

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AlCl3 + AgNO3 -> AgCl + Al(NO3)3

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As + NaOH -> Na3AsO3 + H2

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As2O5 + H2O -> H3AsO4

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Au + HCl + HNO3 -> AuCl3 + NO + H2O

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Au + KCN + O2 + H2O -> K[Au(CN)2] + KOH

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Au2O3 -> Au + O2

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Au2S3 + H2 -> Au + H2S

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B2O3 + H2O -> H3BO3

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C7H10N + O2 -> CO2 + H2O + NO2

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C7H16 + O2 -> CO2 + H2O

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C7H6O2 + O2 -> CO2 + H2O

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CH4 + O2 -> CO2 +H2O

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CO2 + H2O -> C6H12O6 + O2

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Ca + AlCl3 -> CaCl2 + Al

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Ca(NO3)2 -> CaO + NO2 + O2

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Ca(OH)2 + P4O10 + H2O -> Ca(H2PO4)2

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Ca10F2(PO4)6 + H2SO4 -> Ca(H2PO4)2 + CaSO4 + HF

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Ca3(PO4)2 + C -> Ca3P2 + CO

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Ca3(PO4)2 + H2SO4 -> CaSO4 + H3PO4

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Ca3(PO4)2 + H3PO4 -> Ca(H2PO4)2

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Cu + CO2 + O2 + H2O -> CuCO3⋅Cu(OH)2

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CuSO4 + KCN -> CuCN + K2SO4 + C2N2

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Fe + H2O + O2 -> Fe2O3.H2O

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Fe + H2O -> Fe3O4 + H2

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Fe + O2 -> Fe2O3

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Fe(OH)3 -> Fe2O3 + H2O

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Fe2(SO4)3 + Ba(NO3)2 -> BaSO4 + Fe(NO3)3

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Fe2(SO4)3 + KOH -> K2SO4 + Fe(OH)3

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Fe2O3 + C -> CO + Fe

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Fe2O3 + CO -> Fe + CO2

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Fe2O3 + H2 -> Fe + H2O

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Fe3O4 + H2 -> Fe + H2O

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FeC2O4⋅2H2O + H2C2O4 + H2O2 + K2C2O4 -> K3[Fe(C2O4)3]⋅3H2O

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H3AsO3 -> As2O3 + H2O

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H3BO3 + Na2CO3 -> Na2B4O7 + CO2 + H2O

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H3BO3 -> H4B6O11 + H2O

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H3PO3 -> H3PO4 + PH3

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H3PO4 + (NH4)2MoO4 + HNO3 -> (NH4)3PO4⋅2MoO3 + NH4NO3 + H2O

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H3PO4 + Ca(OH)2 -> Ca(H2PO4)2 + H2O

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H3PO4 + HCl -> PCl5 + H2O

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HCl + HNO3 -> NOCl + Cl2 + H2O

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HCl + K2CO3 -> KCl + H2O + CO2

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HClO4 + P4O10 -> H3PO4 + Cl2O7

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Hg(OH)2 + H3PO4 -> Hg3(PO4)2 + H2O

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Hg2CrO4 -> Cr2O3 + Hg + O2

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MnO2 + KOH + O2 -> K2MnO4 + H2O

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NH3 + NO -> N2 + H2O

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NH3 + O2 -> HNO2 + H2O

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NH3 + O2 -> NO + H2O

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NH4Cl + Ca(OH)2 -> CaCl2 + NH3 + H2O

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NH4VO3 -> V2O5 + NH3 + H2O

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NO + NaOH -> NaNO2 + H2O + N2O

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Na + H2O -> NaOH + H2

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Na2B4O7 + HCl + H2O -> NaCl + H3BO3

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Na2CO3 + HCl -> NaCl + H2O + CO2

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Na2O2 + H2O -> NaOH + O2

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Na2S2 + O2 -> Na2S2O3

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Na2SnO3 + H2S -> SnS2 + NaOH + H2O

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PCl5 + H2O -> H3PO4 + HCl

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PCl5 + P2O5 -> POCl3

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POCl3 + H2O -> H3PO4 + HCl

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Pb + Na + C2H5Cl -> Pb(C2H5)4 + NaCl

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Pb(NO3)2 -> PbO + NO2 + O2

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Pb(OH)2 + NaOH -> Na2PbO2 + H2O

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Pb3(VO4)2⋅PbCl2 + HCl -> VO2Cl + PbCl2 + H2O

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Pb3O4 + HNO3 -> Pb(NO3)2 + PbO2 + H2O

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S8 + O2 -> SO3

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Sb + O2 -> Sb4O6

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Se + NaOH -> Na2Se + Na2SeO3 + H2O

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U3O8 + HNO3 -> UO2(NO3)2 + NO2 + H2O

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UO2 + HF -> UF4 + H2O

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UO2(NO3)2⋅6H2O -> UO3 + NO2 + O2 + H2O

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V2O5 + Al -> Al2O3 + V

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V2O5 + Ca -> CaO + V

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V2O5 + HCl -> VOCl3 + H2O

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VO2Cl + NH4OH -> NH4VO3 + NH4Cl + H2O

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Zn + NaOH + H2O -> Na2Zn(OH)4 + H2

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[Ag(NH3)2]Cl + HNO3 -> NH4NO3 + AgCl

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(CN)₂ + NaOH → NaCN + NaOCN + H₂O

1 (CN)₂ + 2 NaOH → 1 NaCN + 1 NaOCN + 1 H₂O

(NH₄)₂SO₄ + CaCO₃ → (NH₄)₂CO₃ + CaSO₄

1 (NH₄)₂SO₄ + 1 CaCO₃ → 1 (NH₄)₂CO₃ + 1 CaSO₄

AgBr + Na₂S₂O₃ → Na₃[Ag(S₂O₃)₂] + NaBr

1 AgBr + 2 Na₂S₂O₃ → 1 Na₃[Ag(S₂O₃)₂] + 1 NaBr

Al(OH)₃ + NaOH → NaAlO₂ + H₂O

1 Al(OH)₃ + 1 NaOH → 1 NaAlO₂ + 2 H₂O

AlN + H₂O → NH₃ + Al(OH)₃

1 AlN + 3 H₂O → 1 NH₃ + 1 Al(OH)₃

Al₂O₃ + Na₂CO₃ → NaAlO₂ + CO₂

1 Al₂O₃ + 1 Na₂CO₃ → 2 NaAlO₂ + 1 CO₂

As₂O₃ + H₂O → H₃AsO₃

1 As₂O₃ + 3 H₂O → 2 H₃AsO₃

BaCO₃ + HNO₃ → Ba(NO₃)₂ + CO₂ + H₂O

1 BaCO₃ + 2 HNO₃ → 1 Ba(NO₃)₂ + 1 CO₂ + 1 H₂O

BaO + H₂O → Ba(OH)₂

1 BaO + 1 H₂O → 1 Ba(OH)₂

BaO₂ + H₂SO₄ → BaSO₄ + H₂O₂

1 BaO₂ + 1 H₂SO₄ → 1 BaSO₄ + 1 H₂O₂

Be(OH)₂ → BeO + H₂O

1 Be(OH)₂ → 1 BeO + 1 H₂O

BeF₂ + Mg → MgF₂ + Be

1 BeF₂ + 1 Mg → 1 MgF₂ + 1 Be

BeO + C + Cl₂ → BeCl₂ + CO

1 BeO + 1 C + 1 Cl₂ → 1 BeCl₂ + 1 CO

BeSO₄ + NH₄OH → Be(OH)₂ + (NH₄)₂SO₄

1 BeSO₄ + 2 NH₄OH → 1 Be(OH)₂ + 1 (NH₄)₂SO₄

C + H₂O → CO + H₂

1 C + 1 H₂O → 1 CO + 1 H₂

CO₂ + NH₃ + H₂O → NH₄HCO₃

1 CO₂ + 1 NH₃ + H₂O → 1 NH₄HCO₃

CO₂ + NH₃ → OC(NH₂)₂ + H₂O

1 CO₂ + 2 NH₃ → 1 OC(NH₂)₂ + 1 H₂O

Ca(ClO₃)₂ → CaCl₂ + O₂

1 Ca(ClO₃)₂ → 1 CaCl₂ + 3 O₂

Ca(HCO₃)₂ → CaCO₃ + CO₂ + H₂O

1 Ca(HCO₃)₂ → 1 CaCO₃ + 1 CO₂ + 1 H₂O

Ca(OH)₂ + CO₂ → CaCO₃ + H₂O

1 Ca(OH)₂ + 1 CO₂ → 1 CaCO₃ + 1 H₂O

Ca(OH)₂ + H₃PO₄ → CaHPO₄ + H₂O

1 Ca(OH)₂ + 1 H₃PO₄ → 1 CaHPO₄ + 2 H₂O

Ca(OH)₂ + CO₂ → Ca(HCO₃)₂

1 Ca(OH)₂ + 2 CO₂ → 1 Ca(HCO₃)₂

CaC₂ + H₂O → C₂H₂ + Ca(OH)₂

1 CaC₂ + 2 H₂O → 1 C₂H₂ + 1 Ca(OH)₂

CaO + C → CaC₂ + CO

1 CaO + 3 C → 1 CaC₂ + 1 CO

CaS + H₂O → Ca(OH)₂ + H₂S

1 CaS + 2 H₂O → 1 Ca(OH)₂ + 1 H₂S

CaSO₄ → CaS + O₂

1 CaSO₄ → 1 CaS + 2 O₂

Ca₃(PO₄)₂ + H₂SO₄ → CaSO₄ + Ca(H₂PO₄)₂

1 Ca₃(PO₄)₂ + 2 H₂SO₄ → 2 CaSO₄ + 1 Ca(H₂PO₄)₂

CdSO₄ + H₂S → CdS + H₂SO₄

1 CdSO₄ + 1 H₂S → 1 CdS + 1 H₂SO₄

CuSO₄ + KCN → Cu(CN)₂ + K₂SO₄

1 CuSO₄ + 2 KCN → 1 Cu(CN)₂ + 1 K₂SO₄

FeS + H₂SO₄ → H₂S + FeSO₄

1 FeS + 1 H₂SO₄ → 1 H₂S + 1 FeSO₄

Fe₂O₃ + SiO₂ → Fe₂Si₂O₇

1 Fe₂O₃ + 2 SiO₂ → 1 Fe₂Si₂O₇

Hg₂CO₃ → Hg + HgO + CO₂

1 Hg₂CO₃ → 1 Hg + 1 HgO + 1 CO₂

H₃PO₄ + Ca(OH)₂ → CaHPO₄⋅2H₂O

1 H₃PO₄ + 1 Ca(OH)₂ → 1 CaHPO₄⋅2H₂O

H₄As₂O₇ → As₂O₅ + H₂O

1 H₄As₂O₇ → 1 As₂O₅ + 2 H₂O

K₂O + H₂O → KOH

1 K₂O + 1 H₂O → 2 KOH

Li₂O + H₂O → LiOH

1 Li₂O + 1 H₂O → 2 LiOH

MnO₂ + K₂CO₃ + KNO₃ → K₂MnO₄ + KNO₂ + CO₂

1 MnO₂ + 1 K₂CO₃ + 1 KNO₃ → 1 K₂MnO₄ + 1 KNO₂ + 1 CO₂

MnS + HCl → H₂S + MnCl₂

1 MnS + 2 HCl → 1 H₂S + 1 MnCl₂

Mn₂O₃ + Al → Al₂O₃ + Mn

1 Mn₂O₃ + 2 Al → 1 Al₂O₃ + 2 Mn

NH₃ + O₂ → HNO₃ + H₂O

1 NH₃ + 2 O₂ → 1 HNO₃ + 1 H₂O

NH₄NO₃ → N₂O + H₂O

1 NH₄NO₃ → 1 N₂O + 2 H₂O

Na₂Cr₂O₇ + S → Cr₂O₃ + Na₂SO₄

1 Na₂Cr₂O₇ + 1 S → 1 Cr₂O₃ + 1 Na₂SO₄

Na₂O + H₂O → NaOH

1 Na₂O + 1 H₂O → 2 NaOH

Na₂SO₃ + S → Na₂S₂O₃

1 Na₂SO₃ + 1 S → 1 Na₂S₂O₃

N₂ + H₂ → NH₃

1 N₂ + 3 H₂ → 2 NH₃

N₂O₃ + H₂O → HNO₂

1 N₂O₃ + 1 H₂O → 2 HNO₂

N₂O₅ + H₂O → HNO₃

1 N₂O₅ + 1 H₂O → 2 HNO₃

PCl₅ + H₂O → POCl₃ + HCl

1 PCl₅ + 1 H₂O → 1 POCl₃ + 2 HCl

PCl₅ + KNO₂ → NOCl + POCl₃ + KCl

1 PCl₅ + 1 KNO₂ → 1 NOCl + 1 POCl₃ + 1 KCl

SiO₂ + Ca(OH)₂ → CaSiO₃ + H₂O

1 SiO₂ + 1 Ca(OH)₂ → 1 CaSiO₃ + 1 H₂O

SiO₂ + Na₂CO₃ → Na₂SiO₃ + CO₂

1 SiO₂ + 1 Na₂CO₃ → 1 Na₂SiO₃ + 1 CO₂

SrBr₂ + (NH₄)₂CO₃ → SrCO₃ + NH₄Br

1 SrBr₂ + 1 (NH₄)₂CO₃ → 1 SrCO₃ + 2 NH₄Br

UF₄ + Mg → MgF₂ + U

1 UF₄ + 2 Mg → 2 MgF₂ + 1 U

UO₃ + H₂ → UO₂ + H₂O

1 UO₃ + 1 H₂ → 1 UO₂ + 1 H₂O

Xe + F₂ → XeF₆

1 Xe + 3 F₂ → 1 XeF₆

Zn + HCl → ZnCl₂ + H₂

1 Zn + 2 HCl → 1 ZnCl₂ + 1 H₂

Zn + KOH → K₂ZnO₂ + H₂

1 Zn + 2 KOH → 1 K₂ZnO₂ + 1 H₂

Zn(OH)₂ + NaOH → Na₂ZnO₂ + H₂O

1 Zn(OH)₂ + 2 NaOH → 1 Na₂ZnO₂ + 2 H₂O

[Cr(N₂H₄CO)₆]₄[Cr(CN)₆]₃ + KMnO₄ + H₂SO₄ → K₂Cr₂O₇ + MnSO₄ + CO₂ + KNO₃ + K₂SO₄ + H₂O ***This is the mother of all chemical equations***

10 [Cr(N₂H₄CO)₆]₄[Cr(CN)₆]₃ + 1176 KMnO₄ + 1399 H₂SO₄ → 35K₂Cr₂O₇ + 1176 MnSO₄ + 420 CO₂ + 660 KNO₃ + 223 K₂SO₄ + 1879 H₂O

Cu(CN)₂ → CuCN + C₂N₂

2 Cu(CN)₂ → 2 CuCN + 1 C₂N₂

HAsO₂ → As₂O₃ + H₂O

2 HAsO₂ → 1 As₂O₃ + 1 H₂O

HAsO₃ → As₂O₅ + H₂O

2 HAsO₃ → 1 As₂O₅ + 1 H₂O

HIO₃ → I₂O₅ + H₂O

2 HIO₃ → 1 I₂O₅ + 1 H₂O

HNO₂ + O₂ → HNO₃

2 HNO₂ + 1 O₂ → 2 HNO₃

HNO₃ + P₂O₅ → N₂O₅ + HPO₃

2 HNO₃ + 1 P₂O₅ → 1 N₂O₅ + 2 HPO₃

HgO → Hg + O₂

2 HgO → 2 Hg + 1 O₂

H₂ + O₂ → H₂O

2 H₂ + 1 O₂ → 2 H₂O

H₂O₂ → H₂O + O₂

2 H₂O₂ → 2 H₂O + 1 O₂

H₃AsO₄ → As₂O₅ + H₂O

2 H₃AsO₄ → 1 As₂O₅ + 3 H₂O

H₃PO₄ → H₄P₂O₇ + H₂O

2 H₃PO₄ → 1 H₄P₂O₇ + 1 H₂O

K + Br₂ → KBr

2 K + 1 Br₂ → 2 KBr

KHSO₄ → K₂S₂O₇ + H₂O

2 KHSO₄ → 1 K₂S₂O₇ + 1 H₂O

Mg(OH)₂ → (MgOH)₂O + H₂O

2 Mg(OH)₂ → 1 (MgOH)₂O + 1 H₂O

NaHCO₃ → Na₂CO₃ + CO₂ + H₂O

2 NaHCO₃ → 1 Na₂CO₃ + 1 CO₂ + 1 H₂O

Na₂HPO₄ → Na₄P₂O₇ + H₂O

2 Na₂HPO₄ → 1 Na₄P₂O₇ + 1 H₂O

N₂ + O₂ → N₂O

2 N₂ + 1 O₂ → 2 N₂O

writing formulas step 2 look at the periodic table for the oxidation number

2+

writing formulas step #6 reduce the oxidation numbers like they are fractions

2/2 will reduce to 1/1 MgO is the answer

Use the Law of Conservation of Mass to answer the following; mercuric oxide ---> mercury + oxygen HgO ---> Hg + O2 If 27.0 g of mercuric oxide (the red solid compound) is heated and completely decomposes to give the elements oxygen and mercury. 2.0 g of oxygen are produced. How many grams of mercury are produced?

25

Ag₂O --> Ag + O₂

2Ag₂O --> 4Ag + O₂

aluminum + hydrochloric acid yield aluminum chloride + hydrogen gas

2Al + 6HCl --> 2AlCl₃+ 3H₂

hydrogen + nitrogen monoxide yield water + nitrogen

2H₂+ 2NO --> 2H₂O + N₂

K + MgBr₂--> KBr + Mg

2K + MgBr₂--> 2KBr + Mg

Na + H₂O --> NaOH + H₂

2Na + 2H₂O --> 2NaOH + H₂

Mg + N₂ → Mg₃N₂

3 Mg + 1 N₂ → 1 Mg₃N₂

O₂ → O₃

3 O₂ → 2 O₃

Polyatomic Ions

3 or more elements involved Charge is based on how many electrons are lost or gained

If a chemical reaction such as photosynthesis begins with 6 atoms of carbon, how many atoms of carbon should be in the products? 12 atoms of carbon, 6 atoms of carbon, 3 atoms of carbon, or 2 atoms of carbon

6 atoms of carbon

CO₂+ H₂O --> C₆H₁₂O₆ + O₂

6CO₂+ 6H₂O --> C₆H₁₂O₆ + 6O₂

The law of conservation of mass states, if you had 8 atoms of Irons and 6 atoms of oxygens before the reaction you would have to have ___ atoms of Irons and ____ atoms of oxygen after the reaction.

8, 6

single replacement reactions (general form)

A + BC → B + AC or A + BC → C + BA

oxidation or oxidize

A chemical change in which a substance combines with oxygen, as when iron oxidizes, forming rust

molecules

A coefficient in front of a chemical formula tells me the number of ________.

coefficient

A number in front of a chemical formula in an equation. indicates HOW MANY MOLECULES of each reactant and product there are. (everything following a coefficient until it reaches the next symbol must be multiplied by that coefficient)

Atom

A particle that makes up all elements and contains electrons, protons, neutrons, and a nucleus

Cation

A positive ion

chemical equation

A representation of a chemical reaction that uses symbols to show how the compounds and molecules in the reactants form new compounds in the products.

pure substance

A sample of matter, either a single element or a single compound, that has definite chemical and physical properties

subscript

A small number to the right of a symbol that is written below the normal line of letters.

formation of a precipitate

A student mixes two clear solutions. After a few minutes small, solid particles begin to form in the solution and settle to the bottom of the container. Which of the following is evidence that a chemical reaction is happening? color change odor change temperature change formation of a precipitate

the bubbles indicated a chemical change was occuring

A student placed 2 grams of baking soda in a balloon and 100 mL of vinegar in a flask. After stretching the opening of the balloon across the neck of the flask, the student raised it to dump the baking soda into the flask. He immediately observed foaming bubbles in the flask and the balloon began to expand. The student concluded that... - a physical change only was occuring - the bubbles indicated a chemical change was occuring - the baking soda and vinegar were products of a chemical reaction - the gas was oxygen

atoms

A subscript to the right of a chemical symbol tells me the number of ________.

decomposition reactions (general form)

AB → A + B or ABC → A + BC or ABC → AB + C

SIngle Replacement

AB+C=AC+B (you started off with someone and now you are alone)

Double Replacement

AB+CD=AD+CB (elements switch partners)

Stock System

Ag (+1) Cd (+2) Zn (+2) Sc (+3)

3

Aluminum atoms = ________

Ion

An atom that has a positive or negative net electric charge depending on whether it loses or gains electrons.

Molecule

Any group of atoms that are held together by covalent bonds in a gas state

Writing Names step 1 BaF2 write the name of the element with a positive oxidation number

Barium it has a positive oxidation number

writing names final answer

Barium Fluoride

methane

CH₄

CH₄+ O₂--> CO₂+ H₂O

CH₄+2O₂--> CO₂+ 2H₂O

combustion

CO2 (carbon dioxide) is heat which is produced

Law of Conservation of Mass

Calculated in Grams Balanced Equations Matter cannot be created or destroyed in any chemical reaction

24

Carbon atoms = ________

4

Carbon atoms = ________

When you use a formulas and symbols to describe a reaction, it is a ____________________________ .

Chemical Equation

Halogens

Contains nonmetals, 7 valence electrons in it's outermost energy level. Very reactive

Which of the following is a chemical reaction in a word equation; Copper reacts with sunshine to make copper shine Copper reacts with chlorine to form copper chloride Copper + chlorine ---> copper chloride Cu + Cl2 ---> CuCl2

Copper + chlorine ---> copper chloride

Which of the following is a chemical reaction in a sentence; Copper reacts with sunshine to make copper shine Copper reacts with chlorine to form copper chloride Copper + chlorine ---> copper chloride Cu + Cl2 ---> CuCl2

Copper reacts with chlorine to form copper chloride

Which of the following is a chemical reaction in a Formula chemical equation; Copper reacts with sunshine to make copper shine Copper reacts with chlorine to form copper chloride Copper + chlorine ---> copper chloride Cu + Cl2 ---> CuCl2

Cu + Cl2 ---> CuCl2

decane

C₁₀H₂₂

ethane

C₂H₆

propane

C₃H₈

butane

C₄H₁₀

pentane

C₅H₁₂

hexane

C₆H₁₄

heptane

C₇H₁₆

octane

C₈H₁₈

nonane

C₉H₂₀

diatomic molecules (def:)

Elements which combine in pairs only when in "free" state (not in compounds)

Chemical reactions that ABSORBS heat, or take away heat from their surroundings, is called _______________ .

Endothermic reactions

Chemical reactions that RELEASES energy to their surroundings in the form of heat, is called _______________ .

Exothermic reactions

FeCl₃+ NaOH --> Fe(OH)₃+ NaCl

FeCl₃+ 3NaOH --> Fe(OH)₃+ 3 NaCl

Fe₂(C₂O₄)₃ → FeC₂O₄ + CO₂

Fe₂(C₂O₄)₃ → 2 FeC₂O₄ + 2 CO₂

writing names step 2 BaF2 write the first part of the name of the negative element

Fluor

writing names step 3 BaF2 add the ending -ide to the first part of the negative element

Fluoride

EXothermic reaction EX=exit thermo-thermal or heat

GIVES OFF energy in the form of heat. Feels hot.

alkali metals

Group 1, 1 electron in outer level, very reactive, soft, silver, shiny, low density; Lithium, Sodium, Potassium, Rubidium, Cesium, Francium

1

How Many Carbon?

6

How Many Chlorine?

3

How Many Nitrogen?

12

How Many Oxygen?

2

How Many Oxygen?

8

How Many Oxygen?

9

How many Calcium?

4

How many Carbon?

3

How many Chlorine?

2

How many Copper?

12

How many Hydrogen?

2

How many Hydrogen?

24

How many Hydrogen?

3

How many Hydrogen?

1

How many Nitrogen?

12

How many Nitrogen?

4

How many Nitrogen?

6

How many Nitrogen?

1

How many Oxygen?

12

How many Oxygen?

24

How many Oxygen?

36

How many Oxygen?

4

How many Oxygen?

6

How many Oxygen?

9

How many Oxygen?

3

How many Phosphorous?

2

How many Phosphorus?

2

How many Potassium?

6

How many Potassium?

12

How many Sulfur?

15

How many TOTAL atoms are in this chemical formula?

30

How many TOTAL atoms are in this chemical formula?

80

How many TOTAL atoms are in this chemical formula?

10

How many atoms TOTAL are there in this chemical formula?

4

How many chemical formulas are in this chemical equation?

5

How many chemical formulas are in this chemical equation?

1

How many coefficients are in this chemical equation?

1

How many phosphorous?

Diatomic Molecules

Hydrogen Oxygen Fluorine Chlorine Bromine Iodine Nirtogen Exist as molecule instead of single atom

32

Hydrogen atoms = ________

6

Hydrogen atoms = ________

chemical equation

I am a combination of chemical formulas used to describe what happens in a chemical reaction. What am I?

chemical formula

I am a combination of symbols and numbers that represent the number and types of elements (atoms) present in a compound. What am I?

coefficient

I am a number written in front of a chemical formula to show how many molecules of that substance are present.

precipitate

I am a solid that forms as a result of a chemical reaction. I will fall to the bottom of the container. What am I?

compound

I am a substance of two or more elements chemically combined and in a definite proportion. What am I?

chemical change

I am a type of change in which a substance (or substances) is changed into one or more new substances with different properties than the original substances. What am I?

physical change

I am a type of change in which the characteristics of a substance are only changed physically and the original properties stay the same. What am I?

two molecules

If 2 atoms of oxygen are combined with 4 atoms of hydrogen, how many molecules will be formed?

arrow

In a chemical equation the ________ symbol shows a reaction has take place.

True

In a chemical equation, the coefficients tell you the number of molecules of each reactant used and the number of molecules of each product made. - True - False

False

In a chemical equation, the reactants and products can have different numbers of atoms for each element. - True - False

False

In a chemical equation, you can end up with different numbers of atoms of an element on the reactant side for the same element on the product side. - True - False

products

In a chemical reaction the new substances formed are called the ________.

coefficient

In the chemical equation above what is letter "A" pointing to?

subscript

In the chemical equation above what is letter "B" pointing to?

chemical formula

In the chemical equation above what is letter "C" pointing to?

chemical symbol

In the chemical equation above what is letter "D" pointing to?

reactants

In the chemical equation above what is letter "E" pointing to?

products

In the chemical equation above what is letter "F" pointing to?

2

In the equation above, what is the coefficient of the magnesium molecule?

2

In the equation above, what is the subscript of the oxygen molecule?

1

In the table, how many atoms of oxygen are in hydronium?

Hydrogen Peroxide

In the table, what does H2O2 stand for?

Law of Conservation of Mass

In this law the number of atoms in the reactants must be equal to the number of atoms in the product.

chemical equation

Is this a chemical equation or a chemical formula?

balanced

Is this equation balanced or unbalanced? Hint: T-chart!

unbalanced

Is this equation balanced or unbalanced? Hint: T-chart!

3

Lithium atoms = ________

Ionic Compounds

Metal- Nonmetal Transition Metal- Nonmetal Polyatomic Ion-Nonmetal Polyatomic Ion-Metal Polyatomic Ion- Polyatomic Ion

writing formulas step 1 write the symbol of the element with a positive oxidation number Magnesium

Mg

Mg + S → MgS which is oxidized? reduced?

Mg is oxidized S is reduced

writing formulas step #5 elements switch oxidation numbers

Mg2- O2+ (switched)

Na₂SO₄ oxidation numbers?

Na = 1+, O = 2-, S = 6+

products

New substances formed during a chemical reaction are indicated on the right side of the equation and are called ________.

2

Nitrogen atoms = ________

balancing equations step #2 try to get the same element on each side of the arrow to equal. example Na has 1 (left side)-- Na has 2 (right side). We add a 2 in front of the NaOH to make the Na =.

Now everything is equal on the right and left side of the arrow.

diatomic molecules (list)

N₂, O₂, F₂, Cl₂, Br₂, I₂, H₂

writing formulas step 3 write the symbol of the element iwth a negative oxidation number oxygen

O

Which of the following are diatomic molecules; H2O Be12 O2 Z3

O2

chemical symbol

One or two letters used to represent an element.

24

Oxygen atoms = ________

4

Oxygen atoms = ________

6

Oxygen atoms = ________

Covalent Compounds

Prefixes are used 2 or more nonmetals

The two parts chemical reactions are ___________ and ___________.

Reactants and Products

2

Silver atoms = ________

reactants

Substances used during a chemical equation are indicated on the left side of the equation and are called ________.

chemical equation

The ________ ________ identifies the reactants and resulting products.

products

The ________ are formulas written on the right side of the arrow.

reactants

The ________ are the formulas written on the left side of the arrow symbol.

subscript

The ________ shows how many atoms of an element are present in a substance.

yields

The arrow in a chemical equation means ________.

balanced equation

The elements on each side of the = sign are the same

CH4

The following is a model of a molecule of Methane. What is the chemical formula for Methane?

reactants

The starting substances in a chemical reaction are called the ________.

Mass Number

The sum of the protons and neutrons in a nucleus

Law of Conservation of Mass

This law states that, "Matter is not created or destroyed, it only changes form."

2

What coefficient needs to be put in the blank to make this chemical equation balanced? Hint: T-chart

3, 3

What coefficients needs to be put in each blank to make this chemical equation balanced? Hint: T-chart

6, 6, 6

What coefficients needs to be put in each blank to make this chemical equation balanced? Hint: T-chart

yields

What does the arrow in the equation mean?

one

When there is no subscript there is only ________ atom present.

J

Which of the following equations follows the Law of Conservation of Mass?

The model does not show why the atoms are bonding.

Which of the following is a limitation of the model above? - The model does not show what the products of the reaction are. - The model does not show what the reactants of the reaction are. - The model does not show why the atoms are bonding. - The model does not show the number of atoms involved in the reaction.

1, 1, 2, 1

Which of the following sets of coefficients would balance the following equation? - 1, 1, 2, 1 - 1, 2, 1, 2 - 2, 1, 1, 2 - 2, 1, 2, 1

D

Which of these equations shows rust, Fe2O3, forming when oxygen, O2, reacts with iron, Fe?

molecule

a compound made of two or more atoms held together by chemical bonds

chemical formula

a formula that shows the elements in a compound and the ratio of atoms. Atoms are indicated by the element symbols and the number of each type of atom is indicated by a subscript.

period

a horizontal row of elements in the periodic table sharing the same number of electron levels

chemical reaction

a process by which one or more chemical substances are converted into different substances by breaking or forming chemical bonds

composition reactions (def:)

a reaction between two elements, two compounds or an element and a compound to form a new compound

hetrogenous

a solution or mixture that is NOT the same, alike, or uniform througout.

homogenous

a solution or mixture that is the same, alike, and uniform througout.

catalyst

a substance that causes or speeds up a chemical reaction.

catalyst

a substance which speeds up a chemical reaction without being used up in the reaction

family/ group

a vertical column of elements having the same valence electron configuration and similar chemical properties

chemical property

any characteristic of a substance, such as flammability, that indicates whether it can undergo a certain chemical change. examples are reactivity, flammability, oxidation, and stability.

(aq)

aqueous substance

ionic bond

attraction between opposite charges of the ion

redox reactions (def:)

chemical change in which there is a transfer of electrons among bonding atoms

The way atoms are joined together is changed during the ________________________ to make a new substance?

chemical reaction

other types of reactions that are redox reactions

composition, decomposition, single replacement and combustion reactions

hydrate

compound that has water chemically attached MgSo4 * 7H20

The law of _____________________ states that during a chemical reaction, matter can not be created or destroyed, the number and the type of atoms you start with is the the number and the type of atoms you end with.

conservation of matter

During a chemical reaction Atoms aren't created or ____________.

destroyed

Elements that never want to be alone, so they often hang out in PAIRS is called ___________________ .

diatomic molecules

O2, H2,Al2

examples of diatomic molecules

reduction (definition and result)

gain of electrons oxidation number decreases

(g)

gaseous substance

combustion

heat and light are produced

(l)

liquid substance

oxidation (definition and result)

loss of electrons oxidation number increases

Which property of metals allows them to be used to make coins that have the same thickness? - electrical conductivity - density - malleability - specific heat

malleability

The law of conservation of mass states that in a chemical reaction that the _________ DOES NOT CHANGE and the number of _________ DOES NOT CHANGE.

mass, atoms

activity series

metals will only replace other metals that are "less active" than they are

alkane series

methane, ethane, propane, butane, pentane, hexane, heptane, octane, nonane, decane

subscript

number written to the lower right of a chemical symbol. shows the number of atoms of the element that comes before it

Noble Gases

one of the elements of group 18 of the periodic table(helium, neon,argon, krypton, xenon, and radon); noble gases are unreactive

writing formulas step #4 look at the periodic table to find the oxidation number of the next element Oxygen

oxygen is 2-

inhibitor

prevents certain reactions (protects and slows down)

The reactants during the CHEMICAL REACTION turn into the ____________ .

products

reactants and products

reactants are on the left side of the arrow products are on the right side of the arrow

decomposition reactions (def:)

reactions in which a compound breaks down into either the elements that make it up, or into simpler compounds or some of each

double replacement reactions (def:)

reactions in which two ionic compounds exchange their positive or negative parts

single replacement reactions (def:)

reactions involving a compound reacting with an element to yield another compound and another element

combustion (def:)

reactions is which an element or a compound reacts with oxygen (rapidly).

oxidation / reduction reactions (aka)

redox reactions

ENdoTHERMic EN=enter Therm=heat

requires energy in the form of heat. Energy enters. Feels cold to the touch.

(s)

solid substance

CATalyst

substance that SPEEDS up a chemical reaction

composition reactions (aka)

synthesis reactions or combination reactions

oxidation number

tells you how many electrons an atom has gained, lost, or shared to become stable

reactant

the "starting substance(s)" in a chemical reaction

oxidation number

the apparent charge of atoms when in a compound

yeilds

the arrow that shows the changing from the reactant to the product in a chemical equation. (can think of it as meaning "equals")

reactants

the elements or compounds that enter into a chemical reaction. (what goes in)

Reactivity

the likelihood of an element bonding with another to form a new compound.

Balanced Equation

the number of atoms in reactants must equal those in product. Law of Conservation of Matter. (what goes in must come out)

Reactants

the part of a chemical reactions that you start with, the part before the ----> (arrow).

Conservation of Mass

the principle stating that matter may be rearranged but is not created or destroyed during a chemical reaction

Products

the substances that you end up with, the part after the ----> (arrow).

Which remains/stays the same during a chemical reaction, - the temperature of the elements, - the total number of atoms, - the total number of compounds - the heat of the substances

the total number of atoms

Which is evidence that elements can combine to form new compounds? melting a solid a liquid a piece of metal with a magnet two liquids react together to create a solid

two liquids react together to create a solid

All chemical reactions have _______ parts

two,

Combustion

type of synthesis reaction that produces heat and light

←→

used to indicate a "reversible" reaction

used to separate reactants from products

+

used to separate two reactants or two products

ionic bond

usually formed between metals and nonmetal


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