Vocabulary Week 17!!

• reactants

• products

• synthesis

• decomposition

• combustion

• shibboleth

• propitiate

• chortle

• unremitting

• inure

Remember…• Chemical reactions

involve changes with atoms’ electrons

• Nuclear reactions involve changes with atom’s nucleus

• Reactants–Starting

substances in a reaction

–Arrow points away from reactants

• Products–Substances

formed during a reaction

–Arrow points to products

+

Chemical Reactions• Types

1. Synthesis

2. Decomposition

3. Single displacement

4. Double displacement

5. Combustion

Synthesis• Two or more substances react to produce

one product

A + B AB

2Na + Cl2 2NaCl

Decomposition• Single reactant breaks down into two or more

products

AB A + B2 NaN3 → 2 Na + 3 N2

Sodium azide decomposes into nitrogen gas and is used in air bags.

Single Displacement• Atoms of one element replace the atoms of

another element in a compound

A + BX AX + B

Mg + 2HCl MgCl2 + H2Tums is used to neutralize stomach acid

Double Displacement• Exchange of positive ions between substances

AX + BY BX + AYCaCO3 + H2SO3 H2CO3 + CaSO4

Double Replacement• Marble can

become eroded by acid rain. Calcium sulfate, a product, leaves a white coating on the statue.

Combustion• Oxygen combines with a substance and

releases energy (and usually products include carbon dioxide and water)

A + O2 CO2 + H2O + bi-products

C8H18 + O2 CO2 + H2O + energy

Type of Reaction

Example

Synthesis A + B AB

Decomposition AB A + B

Single Replacement A + BX AX + B

Double Replacement AX + BY AY + BX

Combustion A + O2 CO2 + H2O + products

Changes in Matter

• Evidence of chemical reaction:1. Gas is produced2. Color Change3. Change in smell4. Formation of solid—precipitate5. Light is produced6. Temperature change

-exothermic-endothermic

• Some reactions occur in water

• When a solid substance is dissolved in water it is an aqueous solution (aq)

Reactivity Series• Helps determine if a reaction

will occur

• If the single element is higher on the list yes a reaction will occur

• If the single element is lower on the list NO REACTION

Most ActiveLithium

RubidiumPotassiumCalciumSodium

MagnesiumAluminum

ManganeseZincIron

NickelTin

LeadCopperSilver

PlatinumGold A + BX AX + B

Al + PbNO3

1. Al (s) + PbNO3 (aq)

2. Cu (s) + MgSO4

3. Al (s) + SnPO4(aq)

4. Zn (s) + K3PO4(aq)

5. Fe (aq) + KCl (aq)

6. Mg (s) + NaNO3 (aq)

7. Zn (s) + CuCl2 (aq)

8. Na (s) + Au(OH)2 (l)

9. Zn (s) + Cu(NO3)2 (aq)

10. Fe (s) + Ni(ClO3)2 (aq)

11. Au (s) + CaSO4 (aq)

12. Mg (s) + LiBr (aq)

13. Ni (s) + CaSO4 (aq)

14. Al (s) + KClO2 (aq)

15. Mn (s) + Na3PO4 (l)

16. Al (s) + Sn(NO3)2 (aq)

17. Ag (s) + PbCl4 (aq)

18. Zn (aq) + FeI3 (aq)

19. K (s) + Cu(ClO3)2(aq)

20. Pb (s) + Au3(PO4)2 (aq)

Law of Conservation of Mass• Mass/matter can not be created nor destroyed

• Atoms you start with (reactants) must still be there when you end (products)

• This is called balancing the equation

• Mass Reactants = Mass Products

Mg + 2HCl MgCl2 + H2

• Big numbers = Coefficients–can change

• Small numbers = Subscripts–DO NOT CHANGE, if you

change you no longer have the same substance

Steps to balancing equations1. Write formulas for all compounds (sometimes

it is given)

2. Separate Reactants and products by a line

3. Count how many atoms of each element are present on the reactant and the product side (element inventory)

4. Change coefficients so that element inventory is balanced

5. Simplify coefficients

6. Check work

Al + O2 Al2O3

C3H8 + O2 CO2 + H2O

KNO3 KNO2 + O2

O2 + CS2 CO2 + SO2

Cu + H2O CuO + H2

Cu + Cl2 CuCl2

Al(NO3)3+ NaOH Al(OH)3 + NaNO3

Fe + H2SO4 Fe2(SO4)3 + H2

KOH + HBr KBr + H2O

Al + S8 Al2S3

Al(OH)3 + H2CO3 Al2(CO3)3 + H2O

Al(OH)3 + HBr AlBr3 + H2O

Vocab Week 18!Last one this semester!

• single displacement

• double displacement

• reactivity series

• precipitate

• aqueous

• obsequious

• moribund

• winnow

• flaccid

• rife

Na + NaNO3 Na2O + N2

Li + AlCl3 LiCl + Al

NH3 + HCl NH4Cl

FeS2 + O2 Fe2O3 + SO2

sodium hydroxide sodium oxide + water

sodium reacts with water to produce sodium hydroxide and hydrogen gas

carbon tetrahydride reacts with oxygen to produce carbon dioxide and water

chlorine + sodium iodide sodium chloride + iodine

hydrogen chlorite chlorine (III) oxide + water

ammonium phosphate + barium hydroxide ammonium hydroxide + barium phosphate

Type of Reaction

Example

Synthesis A + B AB

Decomposition AB A + B

Single Replacement A + BX AX + B

Double Replacement AX + BY AY + BX

Combustion A + O2 CO2 + H2O + products

1. Ba (s) + O2(g) BaO2 (s)

2. HNO3 (aq) + LiOH(aq) LiNO3(aq) + H2O(l)

3. 2Sb(s) + 3 I2 (g) 2SbI3 (g)

4. C3H8 + O2(g) CO2 (g) + H2O(g)

5. H3PO4(aq)+ LiOH (aq) Li3PO4(aq) + H2O(l)

6. Fe(s) + CuSO4 (aq) FeSO4(aq) + Cu(s)

7. CS2 (g) + O2(g) CO2 (g) + S2(s)