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 + Cl 2  2NaCl

Decomposition Single reactant breaks down into two or more products AB  A + B 2 NaN 3 → 2 Na + 3 N 2 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  MgCl 2 + H 2 Tums is used to neutralize stomach acid

Double Displacement Exchange of positive ions between substances AX + BY  BX + AY CaCO 3 + H 2 SO 3  H 2 CO 3 + CaSO 4

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 + O 2  CO 2 + H 2 O + bi-products C 8 H 18 + O 2  CO 2 + H 2 O + energy

Type of Reaction Example SynthesisA + B  AB DecompositionAB  A + B Single ReplacementA + BX  AX + B Double ReplacementAX + BY  AY + BX CombustionA + O 2  CO 2 + H 2 O + products

Changes in Matter Evidence of chemical reaction: 1.Gas is produced 2.Color Change 3.Change in smell 4.Formation of solid—precipitate 5.Light is produced 6.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 Active Lithium Rubidium Potassium Calcium Sodium Magnesium Aluminum Manganese Zinc Iron Nickel Tin Lead Copper Silver Platinum Gold A + BX  AX + B Al + PbNO 3 

1.Al (s) + PbNO 3 (aq)  2.Cu (s) + MgSO 4  3.Al (s) + SnPO 4 (aq)  4.Zn (s) + K 3 PO 4 (aq)  5.Fe (aq) + KCl (aq) 

6. Mg (s) + NaNO 3 (aq)  7. Zn (s) + CuCl 2 (aq)  8. Na (s) + Au(OH) 2 (l)  9. Zn (s) + Cu(NO 3 ) 2 (aq)  10. Fe (s) + Ni(ClO 3 ) 2 (aq) 

11. Au (s) + CaSO 4 (aq)  12. Mg (s) + LiBr (aq)  13. Ni (s) + CaSO 4 (aq)  14. Al (s) + KClO 2 (aq)  15. Mn (s) + Na 3 PO 4 (l) 

16. Al (s) + Sn(NO 3 ) 2 (aq)  17. Ag (s) + PbCl 4 (aq)  18. Zn (aq) + FeI 3 (aq)  19. K (s) + Cu(ClO 3 ) 2 (aq)  20. Pb (s) + Au 3 (PO 4 ) 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  MgCl 2 + H 2 Big numbers = Coefficients –can change Small numbers = Subscripts –DO NOT CHANGE, if you change you no longer have the same substance

Steps to balancing equations 1.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 + O 2  Al 2 O 3 C 3 H 8 + O 2  CO 2 + H 2 O

KNO 3  KNO 2 + O 2 O 2 + CS 2  CO 2 + SO 2

Cu + H 2 O  CuO + H 2 Cu + Cl 2  CuCl 2

Al(NO 3 ) 3 + NaOH  Al(OH) 3 + NaNO 3 Fe + H 2 SO 4  Fe 2 (SO 4 ) 3 + H 2

KOH + HBr  KBr + H 2 O Al + S 8  Al 2 S 3

Al(OH) 3 + H 2 CO 3  Al 2 (CO 3 ) 3 + H 2 O Al(OH) 3 + HBr  AlBr 3 + H 2 O

Vocab Week 18! Last one this semester! single displacement double displacement reactivity series precipitate aqueous obsequious moribund winnow flaccid rife

Na + NaNO 3  Na 2 O + N 2 Li + AlCl 3  LiCl + Al

NH 3 + HCl  NH 4 Cl FeS 2 + O 2  Fe 2 O 3 + SO 2

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 SynthesisA + B  AB DecompositionAB  A + B Single ReplacementA + BX  AX + B Double ReplacementAX + BY  AY + BX CombustionA + O 2  CO 2 + H 2 O + products

1.Ba (s) + O 2(g)  BaO 2 (s) 2.HNO 3 (aq) + LiOH (aq)  LiNO 3 (aq) + H 2 O (l) 3.2Sb (s) + 3 I 2 (g)  2SbI 3 (g) 4.C 3 H 8 + O 2(g)  CO 2 (g) + H 2 O (g)

5. H 3 PO 4 (aq) + LiOH (aq)  Li 3 PO 4 (aq) + H 2 O (l) 6. Fe (s) + CuSO 4 (aq)  FeSO 4 (aq) + Cu (s) 7. CS 2 (g) + O 2(g)  CO 2 (g) + S 2(s)