Naming and Writing Formulas - PowerPoint PPT Presentation

1 / 37
About This Presentation
Title:

Naming and Writing Formulas

Description:

Naming and Writing Formulas More practice 1. oxalate combined with potassium K1+ C2O42- K2C2O4 2. barium bromate Ba2+ BrO31- Ba(BrO3)2 ... – PowerPoint PPT presentation

Number of Views:144
Avg rating:3.0/5.0
Slides: 38
Provided by: RuthH156
Category:

less

Transcript and Presenter's Notes

Title: Naming and Writing Formulas


1
Naming and Writing Formulas
2
Binary Ionic or covalent
  • Binary compounds
  • (Compounds with just two elements)
  • ALL Binary compounds have a suffix IDE on the
    second element name
  • (hydride, oxide, sulfide nitride.)
  • REMEMBER
  • Ionic metal and nonmetal
  • Covalent nonmetal and nonmetal

3
Naming Binary Covalent compounds
  • Numerical prefixes are used to name covalent
    compounds of two elements
  • First element can have any prefix EXCEPT mono
  • Second element will always have both a prefix
    and a suffix

Number of atoms Prefix 1
Mono 2
Di- 3 Tri-
4 Tetra- 5
Penta- 6
Hexa- 7
Hepta- 8 Octa-
9 Nona- 10
Deca-
4
Binary Covalent
  • Binary compounds (Compounds with just two
    elements) H2S
  • 1. Name the first element adding the correct
    prefix (IF NEEDED) di Hydrogen
  • 2. Name the root of the second element, adding
    the correct prefix mono Sulf
  • 3. Add the ending IDE to the root
  • dihydrogen monosulfide

5
What about covalent compounds?
  • Many covalent compounds are named with prefixes.
  • Examples
  • CO2
  • SO2
  • H2O5

carbon dioxide
sulfur dioxide
dihydrogen pentoxide
6
Many covalent compounds are hydrocarbons with
special names
  • Examples
  • CH4
  • C2H6
  • C2H4
  • C2H2

methane
ethane
ethene
ethyne, or acetylene
7
Naming Ionic Compounds
  • Binary compounds (Compounds with just two
    elements) Na2S
  • 1. Name the first element - Sodium
  • 2. Name the root of the second
    element Sulf
  • 3. Add the ending ide to the root
  • Sodium Sulfide

ALL binary compounds will end with ide. There
is an exception compounds with ammonium can
also end in ide.. Ammonium Bromide
8
Naming ionic compounds
  • The first name is the name of the cation
  • Example CaCl2 has first name calcium
  • The last name has the name of the anion. (Anion
    names always end in ide unless they are from
    your polyatomic ion chart.)
  • Example CaCl2 has last name chloride,
  • so CaCl2 is calcium chloride

9
Name these ionic compounds
barium flouride
  • 1. BaF2
  • 2. K2Se
  • 3. CaS
  • 4. AlF3
  • 5. LiH

potassium selenide
calcium sulfide
aluminum flouride
lithium hydride
10
Atoms and Charges
  • Barium Flouride
  • BaF2
  • Barium 1 atom, 2
  • 1 x (2) 2
  • Flourine 2 atoms, -1
  • 2 x (-1) -2
  • (2) (-2) 0
  • Charges balance !
  • Calcium Phosphide
  • Ca3P2
  • Calcium 3 atoms, 2
  • 3 x (2) 6
  • Phosphorous 2 atoms -3
  • 2 x (-3) - 6
  • (6) (-6) 0
  • Charges balance !

11
Ionic Compounds
  • Some common Cations
  • Name and Symbol Ion charge
  • Cesium ion, Cs 1
  • Lithium ion, Li 1
  • Potassium ion, K 1
  • Rubidium ion, Rb 1
  • Sodium ion, Na 1
  • Barium ion, Ba 2
  • Beryllium ion, Be 2
  • Calcium ion, Ca 2
  • Magnesium ion, Mg 2
  • Strontium ion, Sr 2
  • Aluminum ion, Al 3
  • Some common Anions
  • Name and Symbol Ion charge
  • Fluorine, F FluorIDE - 1
  • Chlorine, Cl ChlorIDE - 1
  • Bromine, Br BromIDE - 1
  • Iodine, I IodIDE - 1
  • Oxygen, O OxIDE - 2
  • Sulfur, S SulfIDE - 2
  • Nitrogen, N NitrIDE - 3

12
Some cation names must show their charge
  • Transition metals may form several different
    cations each with a different charge because they
    have more than one oxidation number
  • These cations must have a Roman Numeral in their
    name. The Roman Numeral shows the cations
    charge.

13
Naming Binary Ionic Using Transition metals
  • 1. Identify the cation (IF it is a transition
    look at second element)
  • 2. Identify the oxidation of the second element.
  • 3. Multiply oxidation (of 2nd element) by of
    atoms (for total charges)
  • 4. Use this total to identify oxidation of
    transition metal.

14
Formulas with transition metals..
  • Fe2O3 - Fe Yikes a transition!
  • Look at the element combined with Fe.
  • Oxygen forms a -2 ion , if there are 3 atoms each
    with a -2 charge there is a total charge of -6
    .
  • So if Iron has 2 atoms, the total charge must
    equal 6.
  • Then this iron must be have a 3 oxidation (3
    X 2 6), so it is named Iron (III) Oxide

15
Some Transition Metal Cations
  • Ion name Symbol
  • Copper (I) Cu 1
  • Copper (II) Cu 2
  • Iron (II) Fe 2
  • Iron (III) Fe 3
  • Nickel (II) Ni 2
  • Nickel (III) Ni 3
  • Lead (II) Pb 2
  • Lead (IV) Pb 4
  • Mercury (I) Hg 1
  • Mercury (II) Hg 2
  • Gold ((I) Au 1
  • Gold (III) Au 3
  • Ion name Symbol
  • Chromium (II) Cr 2
  • Chromium (III) Cr 3
  • Tin (II) Sn 2
  • Tin (IV) Sn 4
  • Titanium (II) Ti 2
  • Titanium (III) Ti 3
  • Titanium (IV) Ti 4
  • Manganese (II) Mn 2
  • Manganese (III) Mn 3
  • Manganese (IV) Mn 4
  • Manganese (VI) Mn 6
  • Manganese (VII) Mn 7

16
Ternary compounds contain 3 elements
  • Compounds containing polyatomic ions have charges
    listed on your polyatomic ion chart.

17
Naming non-binary compounds (polyatomics)
  • NaNO3
  • 1.Use the first element name
  • Na - Sodium
  • 2. Add the polyatomic name
  • CHECK YOUR LIST
  • NO3 - Nitrate
  • NaNO3 -

Sodium Nitrate
18
Polyatomic Ion Names
  • Most normal polyatomic ion names will have a
    suffix of ATE
  • ATE suffix indicates Oxygen in formula
  • ITE suffix has one less Oxygen atom than the
    normal
  • Add a prefix of HYPO - has two less Oxygen atoms
    than normal
  • Prefix of PER with normal ADD 1 oxygen atom

19
Example of Polyatomics ate ite hypo - per
  • Note Oxidation DOES NOT change
  • Regular Chlorate - ClO3
  • One less Oxygen Chlorite - ClO2
  • Two less Oxygen Hypochlorite ClO
  • One more Oxygen Perchlorate - ClO4

20
With transition elements
  • You will have to look at oxidation number of the
    polyatomic
  • Follow rules for using transition elements

21
Name these..
Magnesium nitrate
  • Mg(NO3)2
  • Pb(OH)2
  • CuCO3
  • K3PO4
  • NH4Cl

Lead (II) hydroxide
Copper (II) carbonate
Potassium phosphate
Ammonium chloride
22
Check your understanding
  • ASSIGNMENTS
  • Naming of Non-Binary Compounds
  • Naming Compounds (Mixed) Use flow chart
  • Binary Covalent prefixes, IDE suffix
  • Binary Ionic NO prefixes, IDE suffix
  • Ionic with transitions Roman Numerals
  • and IDE suffix
  • Non-Binary use polyatomic list

23
Names of Acids
  • 1. H in binary (an ide) compound acid name
    with prefix Hydro
  • HCl (Hydrogen chloride) aka Hydrochloric
    Acid
  • 2. H with ate polyatomic, use suffix ic
  • HNO3 is nitric acid
  • 3. H with ite polyatomic, use suffix ous
  • H2SO3 is sulfurous acid

24
Writing Formulas
  • Binary Covalent
  • Binary Ionic
  • Binary Ionic (metals with various oxidation
    numbers)
  • Ternary (with polyatomics)

25
Writing Formulas
  • General rules to remember
  • 1. Ide suffix means only 2 elements
  • 2. Use prefixes for covalent (di, tri,)
  • 3. Roman numeral IS the oxidation
  • 4. Ate, ite suffix or Hypo, per prefix use the
    polyatomic list.
  • 5. REMEMBER cation always goes first
  • 6. Reduce when possible

26
Quick try.
  • Write formulas for binary compounds when given
    the oxidation number
  • Na 1 , Cl -1
  • NaCl
  • Ba 2 , N -3
  • 2 X3, -3 x2 so.
  • Ba3N2

27
With Polyatomics
  • REMEMBER a polyatomic is treated as one
    substance with its own charge.
  • Formula for Lithium phosphate
  • Lithium 1 Phosphate -3
  • Li 1 (PO4) -3
  • Least common multiple is 3
  • Li 1 x 3 3 (PO4) -3 x1 -3
  • Final formula Li3PO4

28
Writing Formulas Binary Covalent
  • Look at prefixes to determine number of atoms
    (subscripts)
  • Dinitrogen octofluoride
  • Di means two nitrogen N2
  • Octo means eight fluorine F8
  • Formula N2F8

29
Practice writing covalent formulas
  • 1. Dinitrogen monoxide
  • N2O
  • 2. Carbon tetraphosphide
  • CP4
  • 3. Sulfur difluoride
  • SF2

30
Ionic Compounds from name only
  • What is the chemical formula for
  • aluminum fluoride?
  • List symbols oxidation for each ion
  • Al 3 F -1
  • Identify of atoms to balance the formula -
    need total of 3 negative charges to balance with
    Als 3 positive charges.
  • Write chemical formula, using subscripts for of
    atoms for a neutral compound AlF3
  • Reduce if possible and leave the charges off

31
Practice makes perfect only if you practice
perfect!
  • Write formulas for
  • Calcium sulfide
  • Ca2 S2-
  • CaS
  • Potassium oxide
  • K1 O2-
  • K2O

32
For Transition metals
  • REMEMBER the roman numeral tells you the charge
    (oxidation )
  • Follow previous steps for writing ionic formulas
  • Iron (III) oxide
  • This iron has 3 oxidation
  • Oxygen has -2
  • Formula Fe2O3

33
Practice makes perfect only if you practice
perfect!
  • Write formulas for
  • Iron (III) sulfide
  • Fe3 S2-
  • Fe2S3
  • Lead (II) phosphide
  • Pb2 P3-
  • Pb3P2

34
More practice
  • 1. oxalate combined with potassium
  • K1 C2O42-
  • K2C2O4
  • 2. barium bromate
  • Ba2 BrO31-
  • Ba(BrO3)2

35
Check your understanding
  • ASSIGNMENTS
  • Writing formulas
  • Binary with charges given
  • Polyatomic with charges given
  • Mixed with names only
  • Math Skills workbook 9
  • Chemistry workbook mixed

36
Or - the easy way..
  • Use the criss-cross method
  • aluminum fluoride
  • Aluminum has a 3 charge
  • Fluorine has a -1 charge
  • Cross the two
  • 3 -1
  • Al F
  • 1 atom 3 atoms
  • Formula for aluminum fluoride is AlF3

37
For Polyatomic ions..
  • Use the criss-cross method.
  • Calcium nitrate
  • Calcium has a 2 charge
  • Nitrate has a -1 charge
  • Cross the two
  • 2 -1
  • Ca (NO3)
  • 1 atom 2
    atoms
  • Formula for calcium nitrate is Ca (NO3)2
Write a Comment
User Comments (0)
About PowerShow.com