+ ---> name = + ---> name = + ---> name =

Nomenclature Guide (inorganic) Case 1 1. 2. 3. Greek prefixes: - Nonmetal + Nonmetal First element retains its name. Second element gets -ide ending...
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Nomenclature Guide (inorganic) Case 1 1. 2. 3.

Greek prefixes:

- Nonmetal + Nonmetal First element retains its name. Second element gets -ide ending. Use Greek prefixes to identify the # of atoms (ignore the 1st one if it's a '1')

Examples:

N2O = ______________________

1-

6-

2-

7-

3-

8-

4-

9-

5-

101/2-

SO3 = ______________________ Now Try These: carbon dioxide

__________

BrF3 ________________________

diphosphorus pentasulfide __________

N2O 4 ________________________

Case 2 - fixed metal + nonmetal 1. Metal retains its name. 2. Non-metal retains its ionic name.

• make sure ions join to form a neutral compound •

Examples

Na+

Ca+2

+ Cl- ---> ___________

+ Cl- ---> ___________

name = __________________________

name = __________________________

+

---> ___________

name = ___________________________

+

---> ___________

name = ___________________________

+

---> ___________

name = ___________________________

Now Try These: lithium bromide

____________

Al2S 3___________________________

magnesium hydroxide____________

(NH4)2S O3 _______________________

aluminum acetate

Ba(NO3)2 _________________________

____________

Case 3 - variable charge metal + nonmetal 1. Metal gets its charge written w/ Roman # in ( ) after name 2. Non-metal retains its ionic name. Examples: Fe+2

+

Cl-

---> __________

name = _________________________

Fe+3

+

Cl-

---> __________

name = _________________________

+

---> _________

name = _________________________

+

---> _________

name = _________________________

Now Try These: manganese (IV) chloride __________

Cr(OH)3 ______________________

nickel (III) carbonate __________

CuCO3 ______________________

Case 4

- Acids (positive ion = "H+")

1. Drop the ending on the negative ion. The -ate ending changes to -ic acid. The -ite ending changes to -ous acid. The -ide ending uses the prefix hydro- and the suffix -ic acid

Examples:

H2CrO4 = ______________________ HNO2 = ______________________ HCl = ______________________

Now Try These: hydrobromic acid __________ perchloric acid ____________

H3PO3

_____________________

HI __________________________

“hydrates” when ionic substances have water molecules attached, theyʼre called “hydrates” MgSO4 • 3 H2O =

__________________________________

Now Try These: calcium phosphate tetrahydrate = _________________ NaC2H3O2 • 2 H20 = ______________________________________________

Packet #3+ Objectives (know these for quiz...) • know how to name covalent molecules ("case 1") • know the first 10 Greek prefixes • know how to name ionic compounds ("case 2 & 3") as well as hydrates • know how to name acids (need to know those endings!) ("case 4") • know how to determine the # of e- transferred during ionic bonding • know differences between ionic and covalent bonding • know how to draw Lewis dot structures for molecules & ions, including exceptions to octet rule • know the definition of electronegativity, who developed it, and how to calculate ΔEN • know what a "dipole arrow" is, and how to draw them on molecules • know how to determine the geometry and polarity of molecules WS 3.2 answer bank

ammonium hydroxide, ammonium sulfide, boric acid, bromine trifluoride, calcium nitrite, calcium carbonate, calcium fluoride, carbon tetrachloride, copper (II) chloride hexahydrate, hydrosulphuric acid, iron (II) iodate, iron (II) phosphate, lithium oxalate, magnesium sulfate heptahydrate, magnesium thiosulfate, nitric acid, phosphite ion, phosphorus trioxide, potassium bicarbonate, potassium nitrate, sodium bisulfite, sulphur tetrachloride, sulphur trioxide, tin (II) iodide, tin (II) phosphate, vanadium (V) bromate Al(C2H3O2)3, AlI3, BCl3, Ba(CN)2, BrF7, CaH2, Co(NO3)3•4 H2O, CO, CO2, CS2, Cu3(PO4)2, H2C2O4, HClO3, HNO2, H3PO3, Hg3(BO3)2, KClO3, KCN, KOH, NaCl, NaC2H3O2•5 H2O, NH4C2H3O2, PbS, SeS2, Si2O3, Sr(NO3)2, ZnSO4

Video Questions- Bonding

Name ________________________

1. Why are the noble gases chemically inert? ____________________________________________________ 2. How many valence electrons are in sodium? _______ 3. What charge does sodium get when it forms an ion? ________ 4. Chlorine needs to _______ (gain / lose) how many electrons in order to achieve a noble gas configuration? _____ 5. When salt is viewed with an electron microscope, what basic shape does it have? ________________________ 6. When the bulb slowly lights, what does Don Showalter say? (guess:_____ ) a) "Wow!"

b) "Look at that bulb!"

(actual:______ )

c) "Here we go; the bulb is lit"

d) "How about that!"

7. Which of the crystalline substances conducted electricity when in solution? ____________________ 8. The formation of a covalent bond is an __________________ (endothermic / exothermic) process. 9. The N-N triple bond is _______________ (stronger / weaker) than the single N-I bonds in NI3 10. When the nitrogen triiodide ("small brownish pile") explodes, what does Don Showalter say? ______ a) "There it goes!"

b) "Wow, what a reaction!"

c) "Did you see that!?!"

d) "Now my eyebrows are really spiked!"

11. Today's explosive of choice, which is also a fertilizer, is _____________________________________.

Octet Rule:

What Is An Ionic Bond?

How Does An Ionic Bond Form?

Ionic Bonding Diagrams NaCl

CaCl2

Single Covalent Bond

Double Covalent Bond

Al2O 3

Triple Covalent Bond

electronegativity:

developed by: _____________________________________

Δ EN

structure

0.0

0.4

nonpolar covalent

2.0 polar covalent

bond type

4.0 ionic

Valence Shell Electron Pair Repulsion Theory (VSPER) # of e- pairs (regions)

e - geometry

bond angle: _______

bond angle: _______

bond angle: _______

bonding diagram

molecular geometry

(pull the ropes) polarity

example

Exceptions To The Octet Rule

Common Ions To Memorize For Quiz, Honors Chemistry: 1+ ions

1- ions

H+1 hydrogen L i+1 lithium +1 Na sodium K +1 potassium

F -1 C l-1 B r-1 I -1

N H4 + 1

NO2 - 1

nitrite

NO3 - 1

nitrate

C l O- 1 C l O2 - 1

hypochlorite chlorite

C l O3 -1

chlorate

ammonium 2+ ions

Mg2+ magnesium Ca2+ calcium Ba2+ barium

3+ ion Al3+

aluminum

fluoride chloride bromide iodide

C l O4 - 1

perchlorate

I O3 - 1

iodate

OH- 1 C N- 1 HCO3 - 1

hydroxide cyanide bicarbonate

H S O3 - 1

bisulfite

H S O4 - 1

bisulfate

C 2 H 3 O2 - 1

acetate

2- ions O2S2-

oxide sulfide

C O3 2 -

carbonate

S O3 2 -

sulfite

S O4 2 -

sulfate

3- ions N3P 3-

nitride phosphide

P O3 3 -

phosphite

P O4 3 -

phosphate