ob: what are ions, how do they form, why do they form, what happens once they form? take out your...

OB: What are ions, how do they form, why do they form, what

happens once they form?

Take out your reference tables, open to the Periodic Table.

1. All atoms are neutral because they have equal numbers of protons and electrons.

The + charges = the ― charges.

2. All atoms “like” to be neutral, so this is okay.

(peasants are okay being peasants too)

3. All atoms would “prefer” to be more like noble gases when it comes to electron configurations. Given a chance, they will lose or gain some electrons to get that “fancy” noble gas electron configuration.

(peasants also sorta wish they were more noble-like)

4. Noble gases are “noble” because they have completely full electron orbitals. “Noble like means won’t bond, like the nobles of thrones and castles don’t mix with the peasants.

5. Noble gases do not bond because they don’t need to share their electrons with other atoms to “get” full orbitals. They don’t want to lose electrons or gain any either. They’re “perfect” already.

6. Atoms will lose or gain electrons to get a noble gas electron configuration. That’s called being

7. ISOELECTRIC with a noble gas.

Isoelectric DOES NOT MEAN becomes a noble gas, it means getting a

noble gas electron configuration for itself, by losing (or gaining) electrons.

Let’s look at our standard atom, sodium.

Na 2-8-1 This atom has 11 p+, 11e―, and is neutral.

It’s willing to give up this neutrality for a noble gas electron configuration.

*metals always LOSE electrons when they form ions

8. Na 2-8-1 will LOSE one electron, which will give it an electron configuration of 2-8,

9. Which is just like neon, a noble gas. Since electrons are negatively charged, it becomes a sodium +1 ion.

10. The sodium + ion, with 11 p+, but only 10 e―, which gives it an over all charge of +1

Written like this: Na+1

11. Metal atoms will lose one, two or three electrons to get the same electron configuration as a noble gas. They will end up with a

+1, +2, or +3 charge if they lose one, two, or three electrons.Or

12. Non Metal atoms will gain one, two or three electrons to be ISOELECTRIC with a noble gas. They will end up with a

-1, -2, or -3 charge if they gain 1, 2 or 3 electrons.

14. Ions form when a metal can lose electrons and give them to a non metal that can gain the same electrons. Let’s figure out what’s happening

Atom symbol Atom e- config Ion e- config Ion symbol

Li

Na

K

Rb

Be

Mg

Ca

Al

15. First, let’s fill in the red atom electron configurations


Li 2-1

Na 2-8-1

K 2-8-8-1

Rb 2-8-18-8-1

Be 2-2

Mg 2-8-2

Ca 2-8-8-2

Al 2-8-3

Now let’s figure out how many electrons each will lose to become an ION. Fill in the ion electron configurations next.


Li 2-1 2

Na 2-8-1 2-8

K 2-8-8-1 2-8-8

Rb 2-8-18-8-1 2-8-18-8

Be 2-2 2

Mg 2-8-2 2-8

Ca 2-8-8-2 2-8-8

Al 2-8-3 2-8

Last, let’s fill in the symbol for the + ions, and note which noble gas each ion is isoelectric to.


Li 2-1 2 Li+1 (He)

Na 2-8-1 2-8 Na+1 (Ne)

K 2-8-8-1 2-8-8 K+1 (Ar)

Rb 2-8-18-8-1 2-8-18-8 Rb+1 (Kr)

Be 2-2 2 Be+2 (He)

Mg 2-8-2 2-8 Mg+2 (Ne)

Ca 2-8-8-2 2-8-8 Ca+2 (Ar)

Al 2-8-3 2-8 Al+3 (Ne)

All ions must have a noble gas electron configuration. MUST.

16. All metals LOSE electrons to become positive ions.

POSITIVE IONS arecalled CATIONS.

Metals will lose

1, or 2, or 3 electrons to become cations.

They never lose protons or neutrons.

17. They are give up their neutral nature for a positive charge, but get that noble gas electron configuration.

Non metals will GAIN electrons to get a noble gas electron configuration.

Non metals become negative ions.

Non metals become

DOG-IONS (kidding)

18. Non metals

become

ANIONS


F

Cl

Br

I

O

S

N

P

19. Let’s fill in the atom electron configurations first.


F 2-7

Cl 2-8-7

Br 2-8-18-7

I 2-8-18-18-7

O 2-6

S 2-8-6

N 2-5

P 2-8-5

The, figure out how many electrons will be added and do the Ion electron config.


F 2-7 2-8

Cl 2-8-7 2-8-8

Br 2-8-18-7 2-8-18-8

I 2-8-18-18-7 2-8-18-18-8

O 2-6 2-8

S 2-8-6 2-8-8

N 2-5 2-8

P 2-8-5 2-8-8

Finally, Ion symbols, and tell what noble gas these ANIONS are isoelectric to.


F 2-7 2-8 F-1 (Ne)

Cl 2-8-7 2-8-8 Cl-1 (Ar)

Br 2-8-18-7 2-8-18-8 Br-1 (Kr)

I 2-8-18-18-7 2-8-18-18-8 I-1 (Xe)

O 2-6 2-8 O-2 (Ne)

S 2-8-6 2-8-8 S-2 (Ar)

N 2-5 2-8 N-3 (Ne)

P 2-8-5 2-8-8 P-3 (Ar)

All ions must have a noble gas configuration.

20. Metals lose electrons becoming cations.

21. Non-metals gain electrons becoming anions.22. Cations and anions will bond together, the attraction between the positive and negative is great.

23. The bonding requires a balance of positive & negative: for example, Table salt, sodium chloride, NaCl requires only one chlorine anion for each sodium cation (+1 and -1).

Magnesium oxide (+2 and -2) also require a 1:1 ratio of cations to anions.

Think about sodium oxide.

24. OBJECTIVE: naming simple monoatomic ionic compounds

You must have your own reference tables open to the periodic table

now. No calculators needed.

One big chunk of NaCl

Sodium chloride

25. Ionic compounds form when positive cations (metals) come together with negative anions (non-metals) and are wildly attracted due to opposite charge.

26. Cations form when metals transfer electrons to nonmetals, which simultaneously form negative anions.

27. Opposites attract, it’s like love!!!

28. There is ALWAYS a perfect transfer of electrons, and if not, nothing happens.

It’s either perfect, or nothing.

You already know this: see….

NaCl is called sodium chloride, not

Chlorine sodiumide, or sodium chlorine, or anything else silly.

29. There are 2 rules, the first name rule, and the second name rule to naming simple ionic compounds…

30. 1st name rule: name the cation (metal) first, use the atom name

31. 2nd name rule: name the anion second, change the ending to –ide.

Let’s go through all the second names now (say and write):

32. F, Cl, Br, I, O, S, (Se), N, P, and (As)

The ones in the (parenthesis are rare, especially in this class)

F, Cl, Br, I, O, S, (Se), N, P, and (As)

(fluoride, chloride, bromide, iodide, oxide, sulfide, selenide, nitride, phosphide, + arsenide)

33. Name these compounds:

LiBr CaO BeS MgO CsF SrS AlP

LiBr lithium bromide

CaO calcium oxide

BeS beryllium sulfide

MgO magnesium oxide

CsF cesium fluoride

SrS strontium sulfide

AlP aluminum phosphide

35. What happens if we combine something like calcium and chlorine?

Ca+2 ion forms when calcium atoms lose 2 electrons

Combine it with a

Chloride ion, which forms when a chlorine atom gains 1 electron.

2 electrons transfer from calcium do not match up to 1 electron gain by chlorine??

What’s up with this?

36. Ca+2 + Cl-1 cannot be a 1:1 ratio

37. The Ca+2 must transfer 2 electrons to two different chlorines, forming 2 chloride anions.

38. Calcium chloride is therefore: CaCl2

39.Cation

AnionFormula of compound

Name of compound

Na+1 P-3

Ca+2 S-2

Al+3 P-3

Mg+2 Br-1

Al+3 O-2

39.Cation


Name of compound

Na+1 P-3 Na3P Sodium phosphide

Ca+2 S-2 CaS Calcium sulfide

Al+3 P-3 AlP Aluminum phosphide

Mg+2 Br-1 MgBr2 Magnesium bromide

Li+1 O-2 Li2O Lithium oxide

40.Cation


Name of compound

Be+2 F-1

Sr+2 Cl-1

Ba+2 N-3

K+1 I-1

Al+3 O-2

40.Cation


Name of compound

Be+2 F-1 BeF2 Beryllium fluoride

Sr+2 Cl-1 SrCl2 Strontium chloride

Ba+2 N-3 Ba3N2 Barium nitride

K+1 I-1 KI Potasisum iodide

Al+3 O-2 Al2O3 Aluminum oxide

41. Criss Cross Method of nonthinking, but getting it right (if you think about it) What’s the formula for aluminium oxide?

Al+3 O-2

LiCl

CsF

BeO

MgS

MgF2

Ca3P2

Li3P

Na3N

Al2O3

42.

LiCl

CsF

BeO

MgS

MgF2

Ca3P2

Li3P

Na3N

Al2O3

Lithium chloride

Cesium fluoride

Beryllium oxide

Magnesium sulfide

Magnesium fluoride

Calcium phosphide

Lithium phosphide

Sodium nitride

Aluminum oxideHarpo Marx

43. The compounds formed when ions bond together are called

Ionic Compounds44. They have very strong bonds holding them together, so, they have high melting points, and higher boiling points.45. Ionic compounds only form when metals can transfer electrons directly to nonmetals, “perfectly”.

No loose electrons, no IOU electrons ever.

Tonight:

Naming Compounds HW #1+2

due Tuesday

OB: Transitional Metals become ions too. The rules for ionic bonding and naming ionic compounds from the middle of the table.

You must have a reference table out now, open to the periodic

table.

Let’s look quickly at these basic groupings of metals and non metals:

46. Group 1 all make +1 cations, because all LOSE 1 electron in the outer orbital

47. Group 2 all make +2 cations, because they all lose 2 e– from their outer orbital

48. Al makes a +3 cation, because it loses 3 electrons when it forms a cation

49. Group 17 make -1 anions, because they all need to gain 1 electron to become isoelectric to the noble gases.

50. Group 16 all make -2 anions, they all need to gain 2 electrons to fill their outer orbital

51. Group 15 atoms become -3 anions (you probably know why)

We are about to start discussing what we do with those selected oxidation states.

These numbers will be important for a variety of reasons. With the transitional metals, the selected oxidations indicate the charge of the cation that they form.

52. Scandium makes a +3 cation. See that +3 in the corner? That’s what it’s for.

53. Yttrium too, a +3 cation. Peek at zinc, it only makes a +2 cation.

54. The transitional metals make the cations that are indicated, they do not always follow an “isoelectric” rule, like metals we’ve seen in groups 1 and 2 and Al.

55. When the transitional metals form cations and bond to anions they make ionic compounds. Naming these compounds works the same way as the ones you have already met. For example:

56. React these atoms by changing them to ions, write formulas and names…

Sc + Cl Sc+3 + Cl-1 ScCl3

That stuff is called scandium chloride. Try these 2:

57. Zr + P

58. In + F

That stuff is zirconium phosphide

Zr + P Zr+4 + P-3 Zr3P4

In + F In+3 + F-1 InF3

This is indium fluoride

47.88 +2 +3 +4

222-8-10-2

TiTitanium has 3 different positive selected oxidation states. What is possible here?

Turns out that many of the transitional metals, titanium included, can make more than one stable cation.

59.

Titanium can be Ti+2, Ti+3, or Ti+4

How cool is that?

60. Let’s look at each of these atoms and list what cations that they make:

V-23 for example: V+2, V+3, V+4, and V+5

Cr-24

Fe-26

Cu-29

Ga-31

Cd-48

Nb-41

Hg-80

Let’s look at each of these atoms and determine what cations that they make:

V-23 V+2, V+3, V+4, and V+5

Cr-24 Cr+2, Cr+3, and Cr+6

Fe-26 Fe+2 and Fe+3

Cu-29 Cu+1 and Cu+2

Ga-31 Ga+3

Cd-48 Cd+2

Nb-41 Nb+3 and Nb+5

Hg-80 Hg+1 and Hg+2

They make the cations that they do, the reason is that some of these atoms can flex and become stable

cations even if the electrons are not

isoelectric to a noble gas.

They just can. Just Look.

Let’s make some ionic compounds now.

61. Combine gold with chlorine (do both cations, one at a time) Write the formulas

Au + Cl Au+1 + Cl-1

__________

Au + Cl Au+3 + Cl-1 __________

The formulas are not too tough, but what will we call these compounds? They can’t have the same name if they’re different!

Let’s make some ionic compounds now.

Combine gold with chlorine (do both cations, one at a time)

Au + Cl Au+1 + Cl-1 AuCl gold (I) chloride

Au + Cl Au+3 + Cl-1 AuCl3 gold (III) chloride

It’s going to take some Roman Numerals to have these names different. The Roman Numeral matches the cation charge. These are called stock names.

62.Combine every type of manganese cation with bromine. Write formulas and stock names for each one. (fill in ion charges)

Mn + Br

Mn + Br

Mn + Br

Mn + Br

Combine every type of manganese cation with bromine. Write formulas and stock names for each

one. (fill in ion charges)

Mn+2 + Br-1 MnBr2 manganese (II)

bromide

Mn+3 + Br-1 MnBr3 manganese (III)

bromide

Mn+4 + Br-1 MnBr4 manganese (IV)

bromide

Mn+7 + Br-1 MnBr7 manganese (VII)

bromide

63. There are 2 kinds of copper oxide, we saw them both in the chemical and physical changes lab. One was a black powder, one was red. Show the two ways copper and oxygen can combine ionically, write the proper formulas with their stock names.

Cu + O

Cu + O

There are 2 kinds of copper oxide, we saw them both in the chemical and physical changes lab. One was a black powder, one was red. Show the two ways copper and oxygen can combine ionically, write the proper formulas with their stock names.

Cu+1 + O-2 Cu2O

Cu+2 + O-2 CuO

Copper (I) oxide

Copper (II) oxide

Do Not Forget: the roman numeral matches the cation charge!

Last one…

64. Combine

tantalum (Ta-73) + sulfur (S-16)

Ta + S

Last one…

Combine

tantalum (Ta-73) + sulfur (S-16)

Ta+5 + S-2 Ta2S5 tantalum sulfide

No roman numeral needed, because tantalum only makes one cation (like with sodium, we don’t eat any sodium (I) chloride, do we?)

Read the Naming Compounds BASICS.

OB: Table E, the polyatomic ions, making more ionic compounds!

Get out your reference tables, open to page 2.

Ready, set, go!

We now know about the monoatomic ions of the periodic table and how they bond ionically.

We know also about how the funky transitional metals make cations, and how we use roman numerals to give them their stock names.

We even know why noble gases don’t bond with anything else, which is kind of strange since all those atoms gain or lose electrons to get isoelectric to noble gases so that they can bond.

66. Table E shows us a whole bunch of POLYATOMIC IONS. Poly means more than one, atomic means atoms stuck together.

POLYATOMIC IONS are multiple atoms bonded together in certain ways that act as a single charged particle (positive cations, or negative anions).

On table E, these can be +1, +2, -1, -2, or -3.67. They come as a single bunch, they have special names, you never ever change their names. Most end in –ide, like good anions, but some don’t. Why? Because!

Let’s look at Table E now.

68. We’ll start with ammonium.

Ammonium is one nitrogen atom bonded with four hydrogen atoms, but they act as a +1 cation (like sodium or lithium). They just come hand cuffed (bonded) together.

If sodium bonded to chlorine, it bonds into NaCl, in a 1:1 ratio since the +1 charge balances the -1 charge. There is a transfer of one electron from the cation to the anion, and they end up wildly attracted together, making an ionic bond, forming into an ionic compound.

If ammonium bonded to chlorine, it would bond into NH4Cl, also in a 1:1 ratio since the +1 charge balances the -1 charge. There is a transfer of 1 electron from the cation to the anion, and they end up wildly attracted together, making an ionic bond, forming into an ionic compound.

NH4+1

69. Working with the polyatomic ions, remember these rules:

1. Cations still go first, always. Anions still always go second.

2. Never change the name of a table E polyatomic ion.

Right Now, On Table E, write:

Never ever change these names.

70. Let’s bond sodium with the acetate anion: (name then formula)

Na+1 and C2H3O2-1 will form ________________________________________

How about potassium with the cyanide ion

K+1 and CN-1 will form into _______________________________________

Magnesium will bond with the carbonate ion

Mg+2 and CO3-2 will form into ___________________________________

We will skip the other positive polyatomic ions for now.

Let’s bond sodium with the acetate anion:

Na+1 and C2H3O2-1 will form into sodium acetate, written as: NaC2H3O2

How about potassium with the cyanide ion

K+1 and CN-1 will form into potassium cyanide, written as KCN

Magnesium will bond with the carbonate ion

Mg+2 and CO3-2 will form into magnesium carbonate, written as MgCO3

71. These are really easy, except when the polyatomics have to come in multiples, like these:

Magnesium cation + hydroxide ion forms magnesium hydroxide

Mg+2 + OH-1 creates a simple problem for us, because of the NOT 1:1 ratio needed to keep things balanced. Remember, electron transfer must be perfect, and the resulting ionic compound must be neutral electrically.

What can we do? (when in doubt, don’t think, criss cross)

72. Mg+2 + OH-1 becomes Mg(OH)2

We need two hydroxides to pick up one electron each, to bond with one magnesium cation.

This slide is a break slide. This is a lot of chem, and it’s not easy.

Who has a question about Table E?

Who has a question about ions in general?

Who has a question about transitional metal ions?

Who knows the first thing to look at ina compound or formula to tell if the substance is ionic, or is an ionic compound?

Ask now, or hold on…

It’s tricky tricky tricky, because you will forget the parenthesis, or put the parenthesis in every where, even like Na(Cl) because you will like them. Practice, patience, and more practice please. Soon you’ll also do Magnesium (II) oxide, but you shouldn’t.

Here goes, 4 names and formulas, please.

73. Combine (show ions, show formulas, name stock names):

Lithium + the chromate anion

Aluminum + hypochlorite anion

Magnesium + thiocyanate anion

Calcium + the permanganate anion

Combine:

Lithium + the chromate anion form lithium chromate

Li+1 + CrO4-2 Li2CrO4

Aluminum + hypochlorite anion form aluminum hypochlorite

Al+3 + ClO-1 Al(ClO)3

Magnesium + thiocyanate anion form magnesium thiocyanate

Mg+2 + SCN-1 Mg(SCN)2

Calcium + the permanganate anion form calcium permanganate

Ca+2 + MnO4-1 Ca(MnO4)2

74. Try a few more…

What is the formula for beryllium phosphate? ___________________

What’s the formula for sodium hydrogen carbonate? _____________

Formula for ammonium nitrate? _____________________

How about ammonium dichromate? ___________________________

Super hard ones coming now:

Bismuth (V) thiosulfate ________________________________

Cobalt (III) chlorate ________________________________

Try a few more…

What is the formula for

beryllium phosphate? Be3(PO4)2

sodium hydrogen carbonate (bakin’ soda)? NaHCO3

ammonium nitrate? NH4NO3

ammonium dichromate? (NH4)2Cr2O7

Bismuth (V) thiosulfate Bi2(S2O3)5

Cobalt (III) chlorate Co(ClO3)3

Today was hard

Today was a lot

You are a good person

Peace, Love, and Chemistry.

Don’t get disheartened, you’re not supposed to “get it” all yet.

Give it a few days.

Read your BASICS, it’s very special this one.

OB: molecular compounds, naming and formulas, anddetermining how for form

molecular compounds using selected oxidation states.

Periodic tables mandatory now, smile, this is easier than the rest

of the compounds we’ve looked at

75. Ionic compounds form when positive cations combine in proper ratio

with negative anions, attracting each other because of opposite charge.

The compounds must have a cation combining with anions (+ except for that weird ammonium) all cations are metals.

76. With molecular compounds, the easy way to spot them is that there are NO METALS.

Molecular compounds form when 2 or more nonmetals bond together,in proper ratios.

There are NO ions, no ionic bonds either.

They combine by sharing electrons which we’ll learn about later on in the year. They have their own naming system, which is easy if you can count to ten in Latin.

If you can’t, I will teach you in a few slides.

CO2 CO HCl

NH3 CH4 H2O C8H18

There are NO METALS ever in molecular compounds.

77. When two or more non metals bond together they form a molecule.

78. A molecule is the smallest part of a molecular compound.

79. The bonds that hold these atoms together is called a covalent bond.

80. Co- means ___________________

And –valent refers to _______________

81. When 2 or more ions bond, they make ionic bonds, and they form into FORMULA UNITS. We can abbreviate that as ___________

82. NaCl does not come in molecules, since it does not exist as a single particle. It’s a crystal, or dissolved in water. Ionic Compunds do not form molecules.

83. NAMING RULES FOR MOLECULAR COMPOUNDS

If you can remember what CO, CO2, and H2O are, the naming rules are easy

carbon monoxide, carbon dioxide + dihydrogen monoxide

84. 1st name rule: a single atom? Say just the atom name a multiple atom? Say a prefix first

85. Second name rule: always use a prefix

1 MONO

2 DI

3 TRI

4 TETRA

5 PENTA

6 HEXA

7 HEPTA

8 OCTO

9 NON

10 DECA

87. Using the 2 rules, and the Latin Prefixes, name these 10 example molecules.

You will have to name any molecular compound with up to 10 atoms of any kind.

HF

CS2

SO3

CCl4

PF5

SF6

Cl2O8

I4O9

N2F10

Hopefully you got these all correct…

HF

CS2

SO3

CCl4

PF5

SF6

Cl2O8

I4O9

N2F10

Hydrogen monofluoride

Carbon disulfide

Sulfur trioxide

Carbon tetrachloride

Phosphorous pentafluoride

Sulfur hexafluoride

Dichlorine octoxide

Tetraiodine nonoxide

Dinitrogen decafluoride

First name rule for single atom is

say that atom name. Multiple atoms in first name gets a

prefix.

Second name rule says always use a

prefix.

We will practice names to formulas first…

88. Write the formulas for each molecule:

Phosphorous tribromide ____________

Diphosphorous trioxide ____________

Oxygen difluoride _____________

Dihydrogen monoxide ______________

Nitrogen monoxide ______________

We will practice names to formulas first…

88. Write the formulas for each molecule:

Phosphorous tribromide PBr3

Diphosphorous trioxide P2O3

Oxygen difluoride OF2

Dihydrogen monoxide H2O

Nitrogen monoxide NO

89. Now in reverse, name these compounds

NO2 _________________________

CI4 _________________________

N20 _________________________

SO3 _________________________

N2O5 _________________________

HCl _________________________

89. Now in reverse, name these compounds

NO2 nitrogen dioxide

CI4 carbon tetraiodide

N20 dinitrogen monoxide

SO3 sulfur trioxide

N2O5 dinitrogen pentoxide

HCl hydrogen monochloride

Look right now at tables K and LThese are the acids and bases. We will spend about two weeks on what acid and base chemistry is all about, but today we will look at their names, see that their names and formulas are on your reference tables, say the names together, and that’s that.

Also, there are 7 elements that exist NOT as atoms in their natural state. Rather they exist as pairs of atoms, diatomic elements.Mr. Smith taught this to me in the 8th grade at Junior High School 202 in Ozone Park in Queens. I am happy to share his wisdom now.To remember these seven diatomic elements, we will call them the 90.

HONClBrIF twinsH2 O2 N2 Cl2 Br2 I2 F2

91. How do we decide what ratios of nonmetal atoms fit together to make compounds? Why is water H2O and NO OTHER hydrogen-oxygen compounds exist in any other ratio?

Thinking hats on now.

92. Periodic Tables, Selected Oxidation States

These numbers tell us (with some thinking) what ratios are possible, and what ratios cannot create molecules.

Make this chart in your notes:

H O

Write in all of the oxidation states for

each atom.

Write in all of the possible oxidation states from the Periodic Table of the Elements

H O +1 -2 2:1 ratio possible

-1 X: two negatives ≠ 0

94. The only possible combo for H and O to bond is 2:1, which spells in chemistry:

H2O

95. Let’s determine all of the possible carbon and oxygen compounds that could form with their selected oxidation states. Remember: they must sum to zero, but the ARE NOT IONS. These atoms share electrons only.

C O

95. Let’s determine all of the possible carbon and oxygen compounds that could form with their selected oxidation states. Remember: they must sum to zero, but the ARE NOT IONS. These atoms share electrons only.

C O -4 -2 +2 +4

95. Let’s determine all of the possible carbon and oxygen compounds that could form with their selected oxidation states. Remember: they must sum to zero, but the ARE NOT IONS. These atoms share electrons only.There is NO WAY -4 plus -2 can ever sum to zero, this selected oxidation state for carbon is not used in any carbon – oxygen compounds.

C O -4 -2 1:1 is possible

+2 +4 1:2 is also

CO + CO2 are possible, nothing else is according to our periodic table.

96. Let’s do the big one: All Nitrogen + Oxygen Compounds (there are 5)

N O

96. Let’s do the big one: Nitrogen and Oxygen

N O -3 -2 -1 -2 +1 +2 +3 +4 +5

96. Let’s do the big one: Nitrogen and Oxygen

N O -3 -2 -1 -2 +1 +2 +3 +4 +5

2:1 or N2O dinitrogen monoxide

1:1 or NO nitrogen monoxide

2:3 or N2O3 dinitrogen trixoide 1:2 or NO3 nitrogen trixoide

2:5 or N2O5 dinitrogen pentxoide

5 Possible Compounds

Review Class for Naming Compounds

Sit with some new people, and say,

“hello, my name is __________,

let’s work together, okay?”

say your name

Paper, pen, reference tables ONLY. Clear desks now.Number page 1-25

For each slide there are 2 compounds, tell if each is Ionic or Molecular

Write the name or formula for each

Silver iodide CrN

Ionic/Molecular? Ionic/Molecular?

What’s the formula?

What’s the official name?

1-2

Silver iodide CrN

ionic ionic

AgIChromium III

Nitride

1-2

PCl5 PCl3




3-4

PCl5 PCl3

molecular molecular

Phosphorous pentachloride

Phosphorous trichloride

3-4

Dinitrogen monoxide

ScPO4




5-6

Dinitrogen monoxide

ScPO4

molecular ionic

N2OScandiumphosphate

5-6

PtCl4 ClF




7-8

PtCl4 ClF

ionic molecular

Platinum IVchloride

Chlorine monofluoride

7-8

AsF3 Al(ClO)3




9-10

AsF3 Al(ClO)3

molecular Ionic

arsenic trifluoride

aluminum hypochlorite

9-10

nickel (III) bromide

vanadium (V)sulfide


what’s the formula?

what’s the formula?

11-12

nickel (III) bromide

vanadium (V)sulfide

ionic ionic

NiBr3 V2S5

11-12

tantalum chloride

SiO2




14-15

tantalum chloride

SiO2

ionic molecular

TaCl5Silicon dioxide

(AKA sand)

14-15

NaHSO4 N2O5




16-17

NaHSO4 N2O5

ionic/molecular? ionic/molecular?

sodium hydrogen

sulfate

dinitrogen pentoxide

16-17

What are the HONClBrIF twins?

Write the formulas for 2 acids and for 2 bases.

18-19

HONClBrIF reminds you of the 7 diatomic elements, hydrogen, oxygen, nitrogen, chlorine, bromine, iodine and fluorine, all have H2 or Br2 type formulas

Write the formulas for 2 acids and for 2 bases. Tables K + L

18-19

What are all the phosphorous – chlorine compounds?20

What are all the phosphorous – chlorine compounds?

P Cl-3 -1+3 +1+5 +5 +7

PCl3 phosphorous trichloride

PCl5 phosphorous pentachloride

PCl7 phosphorous heptachloride

PCl3 again

PCl5 again

In our class there are only 3 phosphorous – chlorine compounds.

20

Which are correct? If wrong, why are they wrong?

Chromium (IV) sulfideZinc (II) oxide

Carbon pentoxideArgon monofluoride

Hydrogen monochlorideTin (IV) fluoride

Mercury (II) bromideNiobium (II) iodide

Bromine lithideMgBr3

21-24

Which are correct or wrong? If wrong, why?

Chromium (IV) sulfideZinc (II) oxide

Carbon pentoxideArgon fluoride

Hydrogen monochlorideTin (IV) fluoride

Mercury (II) bromideNiobium (II) iodide

Bromine lithideMgBr3

X Cr does +2, +3, +6 ionsX Zn NO roman numeralX carbon makes CO,CO2

X argon doen’t react everYES YES, SnF4 - in toothpasteYES, Hg makes a +2 ionX, Nb only does +3 & +5X, metal first always!X, Mg+2 + Br-1 = MgBr2

21-24

ob: what are ions, how do they form, why do they form, what happens once they form? take out your...

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