What is the difference between Cu 2 O and CuO? Is there any
difference? You may think that there is very little difference
between the two, but there is! Naming compounds very specifically
is important in order to tell the difference between similar
compounds? Cu 2 O Red powder fungicide CuO Black powder Used in
batteries Copper Compounds
Slide 3
What is a cation? Cations positively charged ion How many
electrons does Group 1,2, and 3 lose? Groups 1,2, and 3 lose
electrons Group 1 lose 1 electron Group 2 lose 2 electrons Group 3
lose 3 electrons Remeber Naming Ions?
Slide 4
Anion negatively charged ion Groups 5,6, and 7 generally gain
electrons Group 5 gain 3 electrons Group 6 gain 2 electrons Group 7
gain 1 electron Remember Naming Ions?
Slide 5
Transition metals usually lose electrons, how many electrons
they lose depends on the element You should memorize these metal
ions Table 9.2! Naming Ions
Slide 6
If you actually think about it, it will make sense why some of
the transition elements could have two different ions Ex: Tin (Sn)
forms both a +2 and a +4 cation Why? (Hint: Use the periodic table
and electron configuration.) +2 cation: Sn = [Kr] 5s 2 4d 10 5p 2
loses 2 from the 5p subshell + 4 cation: Sn can lose both the 2
electrons from the 5p subshell AND two electrons from the 5s
subshell to achieve full stability Naming Ions
Slide 7
Writing and naming ionic compounds. Writing and naming covalent
compounds. Learning Objective of the Day:
Slide 8
Ions composed of more than 1 atom You just have to memorize
these Table 9.3 Most end in ite or ate -ite tells you there is 1
less oxygen atom than the ate ending Polyatomic Ions
Slide 9
what do ionic compounds contain? Ionic compounds contain a
metal and a nonmetal How do we name a binary ionic compound (binary
means composed of 2 elements)? Place the cation name first, then
the anion name Usually add ide to the end of the anion name Naming
and Writing Formulas for Ionic Compounds
Slide 10
What would Cs 2 O be? Cesium oxide NaF? Sodium fluoride Cu 2 O
(hint: copper has two possible ions! Which one is it?) Copper ( I )
oxide SnS 2 Tin (IV) Sulfide Mn 2 O 3 Manganese (III) oxide LiCN
Lithium cyanide (NH 4 ) 2 C 2 O 4 Ammonium oxalate (the ide ending
is usually left out if the anion is a polyatomic ion) Naming and
Writing Formulas for Ionic Compounds
Slide 11
To write a formula for a binary ionic compound, we need to go
back to Ch. 7 and balance the charges Ex: iron (III) oxide Fe +3 O
-2 Fe 2 O 3 Ca +2 S -2 Ca 2 S 2 .reduce to CaS Remember crisscross
the charge and reduce subscripts to the lowest whole number ratio
Naming and Writing Formulas for Ionic Compounds
Slide 12
Another wayjust think about how you would balance the charges
out by finding the least common multiple K +1 N -3 We need a 3 to
balance out the +1 on K (1 x 3 =3) and a 1 to balance out the -3 on
N (1 x 3) = 3 So K 3 N Ba +2 S -2 Both have a 2 charge, they
balance each other out BaS Naming and Writing Formulas for Ionic
Compounds
Slide 13
For polyatomic ions, keep the ion together balance the overall
charge of the ion Ex: Ca +2 (NO 3 ) -1 Ca(NO 3 ) 2 Use parentheses
to set off the polyatomic ion only if there is than one of the
polyatomic ion Ex: Li +1 (CO 3 ) -2 Li 2 CO 3 no parentheses
because there is only one polyatomic ion Ex: NH 4 +1 (SO 3 ) -2 (NH
4 ) 2 SO 3 Naming and Writing Formulas for Ionic Compounds
Slide 14
What is a binary molecular compound? A compound composed of 2
elements that are both nonmetals NOT ions Binary compounds can have
2 elements composed in various ways ex: CO and CO 2 or NO and N 2 O
so we cant name them like we did with ionic compounds We need
prefixesprefixes tell us how many atoms of each element are present
in each molecule Naming and Writing Formulas for Molecular
Compounds
Slide 15
Here are a few hints: If there is only 1 atom of the first
element, omit the prefix mono- You will usually add the ide ending
to the second element Ex: CO Carbon monoxide Ex: N 2 O Dinitrogen
monoxide Ex: Cl 2 O 7 Dichlorine heptoxide Ex: BCl 3 Boron
trichloride Naming and Writing Formulas for Molecular
Compounds
Slide 16
Use the prefixes of each element to write the formula (hint:
-mono is left out of the first element if there is only 1 atom) Ex:
carbon monoxide CO Ex: carbon tetrabromide CBr 4 Ex: diphosphorus
trioxide P2O3P2O3 Ex: iodine heptafluoride IF 7 Naming and Writing
Formulas for Molecular Compounds