+DOR: What’s in a name? Write the element symbol WITHOUT the periodic table1) Lithium 6) Magnesium

2) Fluorine 7) Lead

3) Oxygen 8) Manganese

4) Copper 9) Potassium

5) Mercury 10) Iron

+

What’s in a name?

+

LOL

ASAP

FYI

BRB

+Binary Compounds—Writing Chemical formulas

1) Cation, Anion

2) Write oxidation number/charge on each element.

3) Balance charges by the smallest common multiplier between the two elements. Charges must add to 0 for a neutral compound.

4) Add the subscripts for each element in the chemical compound.

+Example 1: Sodium chloride “salt”

+Example 2: Aluminum oxide

+You try…..

1) Magnesium bromide

2) Lithium chloride

+5) If the first element is a transition element, the oxidation number or charge of the element is given by a Roman numeral (I, II, III, IV, etc.) following the element name. Exceptions: Ag+1 and Zn+2—they will always have these charges.

+

1) Magnesium chloride

2) Sodium sulfide

3) Calcium sulfide

4) Potassium bromide

5) Barium chloride

+Example 3: Tin (IV) sulfide

+

You Try…..

1) Zinc oxide2) Mercury (II) fluoride

+Example 4: Iron (III) oxide

+Try…..

1) Calcium chloride

2) Copper (I) oxide

3) Sodium bromide

4) Potassium sulfide

5) Calcium oxide

+Binary Homework—Due Friday 2/8, write chemical formula with chemical name. 1) Iron (II) oxide 2) Potassium bromide

3) Magnesium chloride 4) Chromium (III) oxide

5) Calcium fluoride 6) Iron (III) sulfide

7) Manganese (IV) sulfide 8) Strontium sulfide

9) Zinc bromide 10) Copper (II) oxide

+DOR: Binary Naming

1) Cobalt (II) nitride

2) Calcium chloride

3) Barium sulfide

4) Chromium (VI) oxide

5) Beryllium sulfide

+Binary Compounds—Writing Chemical formulas (Cont.)

6) If a binary compound has a prefix or prefixes in front of an element name, these prefixes are the subscripts for that element in the chemical formula. Prefixes represent the number of element atoms present in a molecule of the chemical compound.

+Prefixes

1 mono 6 hexa

2 di 7 hepta

3 tri 8 octa

4 tetra 9 nona

5 penta 10 deca

+Example 1: Carbon monoxide

+Example 2: Carbon dioxide

+You Try…..

Diphosphorus trioxide

Iodine heptafluoride

Carbon tetrachloride

+Polyatomic Chemical Compounds—Writing Chemical Formulas.

1) Cation, Anion—reference table

2) Write the oxidation number/charge on each element and polyatomic ion.

3) Balance charges by the smallest common multiplier between the cation and anion. Charges must add to 0 for a neutral compound.

4) Add the subscripts for each element/polyatomic ion to the chemical compound.

*Polyatomic ions: place polyatomic ions in parentheses when adding subscript (ex. (NO3)2)

+Example 1: Silver nitrate

+Example 2: Magnesium acetate

+You try…..

1) Ammonium chloride

2) Calcium carbonate

+

1) Potassium sulfate 11. Mercury (II) hydroxide

2) nitrogen dioxide12. Sodium phosphate

3) sulfur tetrabromide 13. Dinitrogen pentaoxide

4) magnesium phosphate 14. Carbon tetrahydride

5) sodium sulfate 15. Calcium nitrate

6) phosphorus pentachloride

7) selenium trichloride

8) chromium (III) nitrite

9) iodine dioxide

10) magnesium hydroxide

+DOR Regular: Chemical Formulas

1) Barium sulfate 2) calcium sulfide

3) Cobalt (II) carbonate 4) sulfur hexafluoride

5) Carbon tetrabromide 6) tin (IV) chloride

7) Potassium chloride 8) zinc fluoride

9) Strontium iodide 10) magnesium carbonate

+Can we go in reverse?

+Binary Compounds: Chemical Nomenclature

1) Write an element’s oxidation number over the element symbol.

2) Cation, Anion—write the element name

3) Add the ending -IDE to the second element/anion

+Example 1: Al2S3

+

+Example 2: LiCl

+Try……

1) MgO

2) CaBr2

+Transition Elements

4) Place a Roman numeral matching the charge/oxidation # on an element after the positive element’s name. Roman numeral is put in () (ex. (II)). Roman numeral indicates the oxidation number on an element can vary.

-Go back to Step #3

+Example 1: CuS

+Example 2: CoBr2

+You Try….

1) SnO

2) CrCl3

+

5) If both elements are found on the RIGHT side of the periodic table, use the appropriate prefix for a given element.

-Go back to Step #3

+Example 1: CO2

+Example 2: CCl4

+You Try….

1) SO2

2) SBr3

+Compounds with Polyatomic Ions: Chemical Nomenclature1) Write oxidation # for each element/polyatomic ion in the formula

2) Write the element and/or polyatomic ion names.

3) If a transition element (an element where the oxidation # varies), use a Roman numeral to indicate an element’s oxidation # in the chemical name.

*NO –IDE ENDING!!!!

+Example 1: ZnCO3

+Example 2: CuSO4

+You Try……Mg(CN)2

Sr(NO3)2

1) Mg(CN)2

2) Sr(NO3)2

+Regular Classwork1) Ni3(PO4)2 6) Mg3N2

2) AgBr 7) BiI3

3) SnCl4

8)(NH4)2SO4

4) (NH4)2 S 9) ZnCO3

5) HgF2 10) Cu2S

+DOR : Nomenclature and Formulas

1) Cobalt (II) carbonate 2) sulfur hexafluoride

3) Tin (IV) chloride 4) calcium sulfide

5) Ammonium phosphate 6) K2S

7) MgF2 8) Al2O3

9) CuO 10) Fe2O3

+Law of Conservation of Matter:

Matter cannot be created or destroyed.

AMOUNT OF REACTANTS = AMOUNT OF PRODUCTS ! ! ! !

+Guidelines for Balancing Chemical Equations: 

1) Do NOT change the subscripts !

2) Every element MUST have the same amount of atoms on both sides of the equation.

3) To balance, coefficients (numbers) are added in front of the chemical formula until we have the same atom amount on both sides of the equation.

4) Once a coefficient is added, go back and check the rest of the equation5) Balance every element EXCEPT Hs and Os. Then balance Hs, Os are balanced last.

6) CHECK EQUATION TO BE SURE EVERYTHING BALANCES/CANCELS OUT ON BOTH SIDES ! ! !

+Example 1:

Mg + HCl è MgCl + H2

+Example 2:

KI (aq) + Pb(NO3)2 è KNO3 + PbI2

+Example 3:

FeI3 + K2SO4 è KI + Fe2(SO4)3

+Practice

1) Zn + CrCl3 è CrCl2 + ZnCl2

 

2) Cu + H2SO4 è CuSO4 + SO2 + H2O

3) LiAlH4 + H2O è LiOH + Al(OH)3 + H2

 

4) CaSO4 + Al(NO3)3 è Ca(NO3)2 + Al2(SO4)3

+Honors Homework

Worksheet