Chemistry 140 - Quiz 3

For non-metals in the Representative groups

# of electrons gained = [8 - Group #] = magnitude of - charge

For metals in the representative group

# of electrons lost = Group # = magnitude of + charge

The magnitude of the charge =

# of electrons lost or gained

Whenever chemical bonding,

# of protons do not change.

Write the chemical formula for ionic compound formed between: Nitrogen and ammonium

(NH4)3N

Ag fixed charge

1+

Group 1A will be

1+ ions.

Determine the number of protons and electrons present in the following ions. a) P^3- b) Mg^2+

a) 15p, 18e b) 12p, 10e

Determine the number of valence electrons present in atoms of each of the following elements. a) 12Mg b) 17Cl c) 34Se

a) 2 b) 7 c) 6

Ba a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 2 b) lose c) 2 lost d) Ba^2+

Ca a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 2 b) lose c) 2 lost d) Ca^2+

Mg a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 2 b) lose c) 2 lost d) Mg^2+

Sr a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 2 b) lose c) 2 lost d) Sr^2+

Be a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 2 b) lose c) 2 lost d) Be^2+

Mg a) valence shell b) valence electrons

a) 3 b) 2

Al a) valence shell b) valence electrons

a) 3 b) 3

Al a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 3 b) lose c) 3 lost d) Al^3+

Ga a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 3 b) lose c) 3 lost d) Ga^3+

Mg Total number of electrons = 12 a) Valence shell = b) Valence electrons =

a) 3rd b) 2

Se a) valence shell b) valence electrons

a) 4 b) 6

Rb a) valence shell b) valence electrons

a) 5 b) 1

N a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 5 b) gain c) 3 gained d) N^3-

P a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 5 b) gain c) 3 gained d) P^3-

S a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 6 b) gain c) 2 gained d) S^2-

Se a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 6 b) gain c) 2 gained d) Se^2-

Te a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 6 b) gain c) 2 gained d) Te^2-

O a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 6 b) gain c) 2 gained d) O^2-

Br a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 7 b) gain c) 1 gained d) Br^-

I a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 7 b) gain c) 1 gained d) I^-

F a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 7 b) gain c) 1 gained d) F^-

How many valence electrons are present in each of the following ions? a) N^3- b) P^3- c) Al^3+ d) Li^+

a) 8 b) 8 c) 8 d) 2

Give the chemical symbol for each of the following ions: a) the ion formed when an aluminum atom loses three electrons b) the ion formed when a sulfur atom gains two electrons

a) Al^3+ b) S^2-

For each of the following pairs of elements, predict the chemical formula of the compound formed when the two elements interact with each other. a) carbon and bromine b) sulfur and chlorine

a) CBr4 b) SCl2

Write the chemical formula for the ionic compound formed from each of the following types of ions. a) Ca^2+ and Cl^- b) Be^2+ and O^2- c) Al^3+ and N^3- d) K^+ and S^2-

a) CaCl2 b) BeO c) AlN d) K2S

CaS a) cation b) cation name c) anion d) anion name e) compound name

a) Ca^2+ b) calcium c) S^2- d) sulfide e) calcium sulfide

CuS a) cation b) cation name c) anion d) anion name e) compound name

a) Cu^2+ b) copper (II) c) S^2- d) sulfide e) copper (II) sulfide

Determine the chemical formulas for the ionic compounds containing the following pairs of ions, one or both of which are polyatomic. a) K^+ and SO4^2- b) Na^+ and NO3^- c) Ca^2+ and OH^- d) NH4^+ and CN^-

a) K2SO4 b) NaNO3 c) Ca(OH)2 d) NH4CN

Give the symbol for each of the following ions. a) lithium atom that has lost one electron b) a phosphorus atom that has gained three electrons c) a bromine atom that has gained one electron d) a barium atom that has lost two electrons

a) Li^+ b) P^3- c) Br^- d) Ba^2+

Determine the chemical formula for the compound that is formed when each of the following types of ions interact. a) Mg^2+ and Cl^− b) Mg^2+ and S^2- c) Mg^2+ and N^3−

a) MgCl2 b) MgS c) Mg3N2

Write the chemical formulas for the following fixed-charge binary ionic compounds, given their names. magnesium oxide sodium sulfide aluminum chloride lithium nitride

a) MgO b) Na2S c) AlCl3 d) Li3N

How many electrons must each of the following atoms lose or gain in order to obtain a noble gas electron configuration and what is the chemical symbol for the ion produced from such loss or gain? a) N b) S c) K d) Mg

a) N^3- b) S^2- c) K^+ d) Mg^2+

Write the chemical formulas for the following variable-charge binary ionic compounds, given their names. nickel(II) chloride nickel(III) chloride chromium(III) oxide chromium(II) oxide

a) NiCl2 b) NiCl3 c) Cr2O3 d) CrO

Classify each of the following species as (1) a cation, (2) an anion, or (3) not an ion. a) Cl^- b) Na^+ c) F d) N^3-

a) anion b) cation c) anion d) anion

Name the following variable-charge binary ionic compounds given their chemical formulas. CuO Cu2O Mn2S3 AuCl3

a) copper (II) oxide b) copper (I) oxide c) manganese (III) sulfide d) gold (III) chloride

Classify each of the following compounds as ionic or molecular for nomenclature purposes. Al2S3 NO2 KF NH4Br

a) ionic b) molecular c) ionic d) ionic

Indicate whether each of the following atoms or ions is (1) a neutral species, (2) a negatively charged species, or (3) a positively charged species. a) contains 5 electrons, 5 protons, and 5 neutrons b) contains 18 electrons, 19 protons, and 20 neutrons c) contains 18 electrons, 20 protons, and 20 neutrons d) contains 36 electrons, 35 protons, and 46 neutrons

a) neutral b) positive c) positive d) negative

Name the following fixed-charge binary ionic compounds given their chemical formulas. KCl MgF2 Na2O Be3N2

a) potassium chloride b) magnesium fluoride c) sodium oxide d) beryllium nitride

Nonmetals

accept valence electrons.

Molecular compounds

aka covalent compounds

Al^3+

aluminum

when using group number to determine valence electrons for main group elements

always use group number w letter next to it. If it doesn't have a letter, don't use it

NH4CN

ammonium cyanide

If the number of protons is less than number of electrons,

anion [overall negative charge]

Ionic compounds are formed between

anions and cations.

Polyatomic ion:

any ion that is made from more than one atom.

Electrons that make a covalent bond

are called shared electrons or bonded electrons

In chemical bonding, the core electrons

are unaffected

Covalent bond is represented

as line between atoms

central atom.

atom capable of making most number of covalent bonds

Covalent bonds are formed when

atoms SHARE pairs of valence electrons by overlap of valence shells so both nuclei can claim all shared electrons to satisfy octet rule.

Chemical Bonds

attractive force that holds 2 atoms together at specific average nuclear distance to serve as part of bigger particle

N3^-

azide

Ba

barium

Ba^2+

barium

Can't look at periodic table for Cu charge

bc it does not have a fixed charge -so start with anion side

How can a Cl atom achieve an octet?

can gain 1 valence electron or lose 7 valence electrons

carbon ion

carbide

Formula unit =

cation + anion

Ionic:

cation + anion

To determine if a compound is ionic ---

cation + anion

CaCl2 cation and anion

cation = Ca^2+ anion = Cl^- Cl^-

Ionic bond is made when

cation combines with anion.

In the chemical formula of ionic compounds,

cation must be written before anion.

NH4^+ is

cation. Will be ionic compound.

All Group IA

charge 1+

Group IIA

charge 2+

Atom is

charge neutral

Compound:

chemical combination of 2 or more diff elements.

Formation/Breaking of a chemical bond is

chemical process that changes chemical identity of substance undergoing change.

CrO3

chromium(VI) oxide

Electron is

constantly moving.

CuCl

copper(I) chloride

CuCl2

copper(II) chloride

Merging of valence shells creates

covalent bond

Non metal atoms bond with each other via

covalent bonding [sharing pairs of valence electrons to satisfy octet rule]

Boron does

covalent bonding.

Molecular compounds have

covalent bonding.

Silicon makes

covalent bonding.

No ions in

covalent bonding. It's only sharing.

Molecular compounds are made through

covalent bonds.

CN^-

cyanide

Variable Charge Cation can have

diff magnitudes of + charge.

Noble=

don't need to react to become stable.

Lewis Symbols for Elements

easy & quick representation of element showing its symbol & valence electrons only.

An ionic compound is formed when

electrons are transferred from metal atom to non-metal atom.

When an ionic bond is created,

electrons are transferred from valence shell of metallic atoms to valence shell of non-metallic atoms

Valence Electrons

electrons in outermost [valence] shell of atom.

alence electrons =

electrons in outermost shell.

the ion representation is only complete when

element symbol AND charge are given

Highest energy =

farthest away, least stable

outermost shell

farthest from nucleus

Cation is written

first, then anion

Ex: NaCl, Al2O3, ZnSO4, NH4CO3

fixed charge cations

The atoms that "loses" electrons

forms a cation

the atom that "gains" electrons

forms an anion.

Non-metallic atoms

gain electrons and make anions.

Non metals

gain valence electrons to make anions

The subscripts in chemical formulas of ionic compounds

give lowest whole number ratio of cations to anions.

To identify ion,

give symbol and its charge.

Au2O3

gold(III) oxide

Formula unit will always

have lowest ratio of cations and anion so overall charge is zero.

hydrogen ion

hydride

H^+

hydrogen ion

OH^-

hydroxide

Energy of shells

increases as go toward outside of atom

If there's no cation, that

indicates there's no anion. This means it's a molecular compound.

Molecular/Covalent compounds

involve covalent bonding

N^3- is

ion; anion; monoatomic ion.

Ionic compounds are made through

ionic bonds.

Ionic compounds are made via

ionic bonds.

Metals always form

ionic compounds.

Example: K2O - Ca2O

ionic compounds:

Compounds can be

ionic or molecular.

FeSO4

iron(II) sulfate

Making a chemical bond

is a chemical process.

Space between 2 nuclei

is most stable space for electrons to be in bc of charges.

Farthest shell =

least stable

In covalent bond,

line represents 2 electrons.

Electrons that are not shared =

lone pairs.

When asked if molecular or ionic compound,

look for a cation

Atoms will either

lose or gain electrons to achieve octet [full valence shell], taking a path that involves FEWER electrons

Metallic atoms

lose valence electrons and make cations.

Metals

lose valence electrons to make cations

For nonmetals =

magnitude of negative charge

For metals =

magnitude of positive charge = group number

Metals

make cations; donate valence electrons

Carbon prefers to

make covalent bonds.

Neutral, uncharged halogens

make single bonds.

Electrons being in pairs

make them more stable.

cation

metal atom/ammonium

Cations will either be

metals or polyatomic cation NH4^+

HCl is a

molecular compound bc no metal/cation or NH4^+

HCl

molecular compound. NOT IONIC.

monoatomic or polyatomic? N^3-

monoatomic

monoatomic or polyatomic? O^2-

monoatomic

monoatomic or polyatomic? Cl^-

monoatomic [made from 1 atom]

Quicker can donate valence electrons,

more metallic it is.

If ends in -ide,

most are monoatomic anions. EXCEPT CN^- , OH^- , N3^-, O2^2-

Closest shell is

most stable shell.

Variable charge:

name of cation is name of element + magnitude

NiBr2

nickel(II) bromide

Molecular:

no ions

anion

non-metal atom[s]

hydrogen is a

nonmetal

Inert = No ions in covalent bonding. It's only sharing.

nonreactive

The shared electrons

now occupy space around both nuclei of 2 atoms.

All atoms have

nucleus [where protons and neutrons live]

Number of electrons contributed by each non-metal atoms =

number of covalent bonds it forms

number of covalent bonds it forms =

number of electrons it needs to satisfy octet rule.

Number of covalent bonds nonmetallic atom wants to make =

number of electrons need to satisfy octet rule.

chlorine wants to make

one

Ionic bond is formed when

one atom donates its valence electrons to valence shell of another atom.

Charge magnitude = 1 =>

one electron was donated

Cl^- =

one ion made from 1 Cl^- atom w overall charge of -1

Cl2^- =

one particle. But is polyatomic ion with -1 overall charge.

Ions are the

only particles to have a charge

cation and anion

oppositely charged ions are electrostatically attracted to each other, forming ionic bond

Valence shell =

outermost shell for atom that has electrons in it. V

Valence Shell

outermost shell of atom that is populated by electrons

C2O4^2- =

oxalate

O^2- =

oxide

O =

oxygen

Isoelectronic particles =

particles that have same number and arrangement of electrons

What will happen if # of p is not equal to # of e?

particles will have net charge -> ions

O2^2-

peroxide

monoatomic or polyatomic? CO3^2-

polyatomic

monoatomic or polyatomic? N3^-

polyatomic

monoatomic or polyatomic? O2^2-

polyatomic

CO3^2- is a

polyatomic ion

Baking soda is a

polyatomic ion.

K^+

potassium

Sodium is

representative element; in period 3 [valence shell is also 3] and group number is 1 [has 1 valence electron]

Variable charge: anion named

same as in fixed charge

Group 1A/1+ ions

same group bc similar chemical property.

Fixed Charge Cation Will have

same magnitude of + charge in all compounds.

Every atom must

satisfy octet rule

In covalent bonds,

shape doesn't matter [horizontal, vertical] - only order matters

In triple bond,

sharing 6 electrons [3 pairs]

One that wants to make the most bonds

should go in middle [be the central atom]

Do not

show charges for formula unit

Ag

silver

AgNO3

silver nitrate

kinds of covalent bonds =

single, double, triple

Na3PO4

sodium phosphate

Shell denotes

space where electrons can be and where most likely are.

SO4^2- =

sulfate

If name of anion ends with ate or ite, i

t's a polyatomic anion.

If it was Al2(O3)3 then

the anion is polyatomic.

So if Cu^1

then copper (I)

If there is a cation,

then it is guaranteed there is an anion also. That is an ionic compound.

2Cl^- =

there are 2 separate Cl^- particles. Each made from one chlorine atom and each has separate charge.

TiPO4

titanium(III) phosphate

The total # of electrons lost by the metallic atom(s) =

total number of electrons gained by the non-metallic atom(s).

Ionic bond:

transferring valence electrons

If it's a polyatomic ion,

use same word or name given in table.

Non-metals Gain valence electrons to make anions

when making a bond w metals

Ca2O2

would be wrong bc not smallest ratio

Helium wants to make

zero bonds

Zn

zinc

Zn^2+

zinc

ZnSO4

zinc sulfate

Give chemical formulas for the compound below: Silver sulfite

Ag2SO3

Silver, cadmium and zinc always have

Ag^+, Cd^+2, Zn^+2 [those are fixed charges]

Lewis symbol for aluminum

Al with 3 dots around it

Write the chemical formula for ionic compound formed between: Aluminum and acetate

Al(C2H3O2)3

oxygen and aluminum

Al2O3

aluminum and selenium =

Al2Se3

chlorine and aluminum

AlCl3

Write the chemical formula for ionic compound formed between: Aluminum and iodine

AlI3

Give chemical formulas for the compound below: Aluminum phosphide

AlP

Write the chemical formula for ionic compound formed between: Aluminum and phosphorus

AlP

aluminum phosphate

AlPO4

Show the ion if: Aluminum atom loses 3 electrons

Al^3+

identify ions in Al2O3

Al^3+ and O^2-

Al

Aluminum

Name the compounds below: Al2O3

Aluminum oxide

Name the compounds below: (NH4)3PO4

Ammonium phosphate

As^3-

Arsenide ion

Octet Rule

Atoms lose, gain or share valence electrons to achieve stable noble gas electronic arrangement

Ionic Bond Model

Attraction between ions w opposite electrical charges

Give chemical formulas for the compound below: Gold (I) phosphide

Au3P

what is the charge of the cation? Au2O3

Au^3+

After the overlap of the valence shells from both atoms,

BOTH nuclei can claim all of shared electrons as own.

Write the chemical formula for ionic compound formed between: Sulfur and barium

BaS

Write the chemical formula for ionic compound formed between: Sulfate and barium

BaSO4

identify ions in Ba(NO3)2

Ba^2+ and NO3^-

Name the compounds below: Ba(C2H3O2)2

Barium acetate

Write the chemical formula for ionic compound formed between: Berillium and nitrite

Be(NO2)2

Write the chemical formula for ionic compound formed between: Beryllium and bromine

BeBr2

Lewis symbol for bromine

Br with 7 dots around it

draw covalent bond for CCl4

C in center, single bond to each Cl, each Cl has 6 electrons around

Draw covalent bond for CH4

C with 4 H connected

Lewis symbol for carbon

C with 4 dots around it

Chemical formula for ionic compound formed between: Calcium and nitrogen

Ca3N2

calcium and oxygen

CaO

Show the ion if: Calcium atom loses 2 electrons

Ca^2+

What ion does calcium form?

Ca^2+

ions in Ca(NO2)2

Ca^2+ and NO2^-

Cd

Cadmium

Name the compounds below: Cd3N2

Cadmium nitride

If the number of protons is greater than number of electrons,

Cation [overall positive charge]

Cd^2+ and PO4^3-

Cd3(PO4)2

Atoms will either lose or gain electrons to achieve an octet (full valence shell) taking a path that involves FEWER electrons. so

Cl atom would gain 1 valence electron [forms Cl^-]

Chloride =

Cl^-

Give chemical formulas for the compound below: Cobalt (II) permanganate

Co(MnO4)2

H-H =

H2 [line represents covalent bond]

Roman numerals in order,

I, II, III, IV, V, VI, VII, VIII, IX, X

Draw covalent bond for iodine and nitrogen

I-N-I I I [N has 2 electrons, each I has 6]

Ionic Compounds with Variable Charge Cations:

Ionic compounds where cations can have diff magnitude of positive charge.

Fe(NO3)3

Iron (III) Nitrate

Name the compounds below: FePO4

Iron(III) phosphate

Write the chemical formula for ionic compound formed between: Potassium and oxygen

K2O

Write the chemical formula for ionic compound formed between: Potassium and phosphate

K3PO4

potassium cyanide

KCN

potassium and chlorine =

KCl

Give chemical formulas for the compound below: Potassium nitrate

KNO3

Identify ions in K2SO4

K^+ and SO4^2-

Pb(CN)2

Lead(II) Cyanide

Name the compounds below: Pb(SO4)2

Lead(IV) sulfate

How would a Li atom achieve an octet?

Li forms Li^+

sulfur and lithium =

Li2S

lithium selenide formula

Li2Se

bond between lithium and bromine

LiBr

ex: formula unit =

LiBr

Chemical formula for ionic compound formed between: Lithium and fluorine

LiF

examples of isoelectronic particles

Li^+ , Be^2+ , He

Name the compounds below: Mn3N2

Manganese(II) nitride

magnesium phosphite formula

Mg3(PO3)2

magnesium and nitrogen =

Mg3N2

Write the chemical formula for ionic compound formed between: Chlorine and magnesium

MgCl2

Identify ions in MoO3

Mo^+6 and O^2-

Name the compounds below: MoO3

Molybdenum(VI) oxide

Cations

Monoatomic or Polyatomic Particle with + charge

Naming ionic compounds:

NAME CATION FIRST AND THEN AS SEPARATE WORD, GIVE NAME OF ANION.

Give chemical formulas for the compound below: Ammonium cyanide

NH4CN

Write the chemical formula for ionic compound formed between: Ammonium and hydroxide

NH4OH

charges of the ions are

NOT written in chemical formulas of ionic compounds

Draw covalent bond for N2

N[triple bond]N [each has 2 electrons around]

Chemical formula for ionic compound formed between: Oxygen and sodium

Na2O

sodium and oxygen

Na2O

Write the chemical formula for ionic compound formed between: Chlorite and sodium

NaClO2

What ion does sodium form?

Na^+

Identify ions in NaCl

Na^+ and Cl^-

Lewis symbol for sodium

Na•

If have Li^+ and Br^1- ions

Need to put together in such way that total positive charge is equal to total negative charge.

In a covalent bond,

Neither atom loses/gains electrons, hence no ions formed

Does a formula unit have a charge?

Never

Does an atom or molecule have a charge?

Never

what is the charge of the cation? NiBr2

Ni^2+

Oxygen gas =

O2

Draw covalent bond for CO2

O=C=O [each O has 4 electrons around]

Draw covalent bond for O2

O=O [each O has 4 electrons around]

In CH3OH ,

OH is NOT an anion bc there is no cation.

In KOH,

OH is an anion bc there is a cation.

What ion does oxygen form?

O^2-

In chemical bonding,

Only valence electrons participate

Show the ion if: Phosphorus atom gains 3 electrons

P^3-

Name the compounds below: K3N

Potassium nitride

Write the chemical formula for ionic compound formed between: Nitrogen and rubidium

Rb3N

Rb

Rubidium

Show the ion if: Sulfur atom gains 2 electrons

S^2-

Covalent Bond:

Sharing of electrons between 2 atoms

Give chemical formulas for the compound below: Tin (IV) cyanide

Sn(CN)4

Go through the process to name Ca3N2

-ionic -fixed charge cation -calcium -monoatomic anion -calcium nitride

Write the chemical formula for ionic compound formed between: Permanganate and strontium

Sr(MnO4)2

If anion is monoatomic anion, it is named as

Stem of element name + replace ending with suffix "ide"

Every shell has

a capacity [max # electrons can hold]

Rb a) valence electrons b) lose or gain electrons c) # of electrons lost/gained d) ion formed

a) 1 b) lose c) 1 lost d) Rb^+

FOR REPRESENTATIVE ELEMENTS ONLY,

-valence shell = period number -valence electrons = group number

The overall charge for each formula unit of an ionic compound =

0

The overall charge of the formula unit =

0

Shell closest to nucleus =

1

Valence electrons for Na

1

Single Bond =

1 Pair of Shared Electrons

Iodine wants to make

1 bond

Acids:

1) "ide" acids 2) "ate" acids 3) "ite" acids

What are the predicted ions for? 1) Ca 2) P 3) I 4) Ga 5) Se 6) K

1) Ca^2+ 2) P^3- 3) I^- 4) Ga^3+ 5) Se^2- 6) K^+

Ionic compounds:

1) Fixed charge cation 2) Variable charge cation

What are the fixed charge cations?

1) Group IA 2) Group IIA 3) Al 4) Ga 5) Zn 6) Cd 7) Ag

Cation comes to you from either

1) Metals 2) NH4^+

Types of cations

1) Metals [Fixed charge cations & variable charge cations] 2) Polyatomic cations [NH4+]

Molecular compounds:

1) Non-acidic 2) Acids

Molecular Compounds can be

1) Non-acidic molecular compounds 2) Acids

For Representative [main Group] Elements:

1) Valence Shell = Period # 2) Valence Electrons = Group #

How do you name an ionic compound with a variable charge cation?

1) cation [no change] & charge in parenthesis + monoatomic anion w suffix ide 2) cation [no change & charge in parenthesis] + polyatomic ion [no change]

How do you name an ionic compound with a fixed charge?

1) cation [no change] + monoatomic anion + suffix ide 2) cation [no change] + polyatomic ion [no change]

Ionic compounds can have

1) fixed charge cations 2) variable charge cations

Is it molecular or ionic compound? 1) KOH 2) NH4OH 3) CH3OH 4) TiOH

1) ionic [cation is K^+ and anion is OH^-] 2) ionic [cation is NH4^+ and anion is OH^-] 3) molecular 4) ionic

Types of Chemical Bonds

1) ionic bond 2) covalent bond

Molecular or ionic? 1) H2SO4 2) FeCl3 3) (NH4)3PO4 4) NaCl 5) HNO3

1) molecular bc hydrogen is nonmetal 2) ionic 3) ionic 4) ionic 5) molecular

How distinguish between molecular and ionic compounds?

-ask yourself is there a cation? LOOK FOR A CATION. -IF YES, there will be an anion. If not, there won't be -therefore, compound is ionic -if no cation, the compound is molecular.

3 possible endings for names of anions:

-ate -ite -ide

Write formula for cadmium phosphate:

-cadmium is fixed charge cation [Cd^2+] -phosphate: polyatomic anion -phosphate: PO4^3- -Cadmium phosphate: Cd3(PO4)2

In Al2O3,

-cation is Al^3+ -anion is O^2-

Go through the process to name Ag2S

-ionic -fixed charge -cation = silver -monoatomic anion -silver sulfide

Go through the process to name ZnSO4

-ionic -fixed charge [Zn^2+] -cation = zinc -polyatomic ion = sulfate -zinc sulfate

go through the process to name Al2O3

-ionic -fixed charge cation -aluminum -O3 means there are 3 oxygens with each a charge of 2- -anion is monoatomic [is each anion monoatomic or polyatomic is the question] -aluminum oxide

Go through the process to name Ca(NO2)2

-ionic -fixed charge cation -calcium -polyatomic anion -calcium nitrite

If it was Al(O2)3

-ionic -fixed charge cation -cation is aluminum -polyatomic anion -aluminum peroxide

KCl go through the process to name it

-ionic -fixed charge cation -cation is potassium -Cl is monoatomic anion so chloride -potassium chloride

anion will be:

1) monoatomic 2) polyatomic

Nuclear charge for sodium atom:

11+

Shell 3 can hold

18 electrons

Ca (Z=20) Valence electrons?

2

Covalent bond is formed when

2 atoms share pairs of valence electrons via overlap of valence shells

Sulfur atom wants to make

2 bonds

Neutral, uncharged oxygen will make

2 bonds [can be one double or 2 single]

each line represents covalent bond

2 electrons

In this case, both H nuclei now have

2 electrons each in valence shell [satisfy Octet Rule]

Shell 1 can only hold

2 electrons.

Double Bond =

2 pairs of shared electrons

Cd fixed charge

2+

Zn fixed charge

2+

Valence shell for Na

3

Neutral, uncharged nitrogen makes

3 bonds [can be 1 triple, 3 single, 1 double + 1 single

Phosphorus atom wants to make

3 bonds.

Triple Bond =

3 pairs of shared electrons

Al fixed charge

3+

Ga fixed charge

3+

Shell 5, 6 etc can hold

32 electrons

Shell 4 can hold

32 electrons.

Ca (Z=20) Valence shell?

4

carbon wants to make

4

Neutral, uncharged, Carbon makes

4 bonds

C would be

4- but mostly does covalent bonding.

O (Z=8) Valence electrons?

6

O (Z=8) Valence shell?

8

Atoms lose, gain or share valence electrons in order to have

8 electrons in outermost shell [except when outermost shell is first shell which cannot hold more than 2 electrons]

Shell 2 can hold

8 max electrons.

# of electrons gained by non-metal atom =

8-Group #

Cu3PO4

Copper (I) Phosphate

Cu2SO4

Copper (I) Sulfate

Give chemical formulas for the compound below: Chromium (II) sulfite

CrSO3

what is the charge of the cation? CrO3

Cr^6+

copper(II) nitrate

Cu(NO3)2

Give chemical formulas for the compound below: Copper (I) hydroxide

CuOH

what is the charge of the cation? CuCl

Cu^+

Identify ions in CuCl

Cu^+ and Cl^-

what is the charge of the cation? CuCl2

Cu^2+

identify ions in CuCl2

Cu^2+ and Cl^-

iron(II) hydroxide

Fe(OH)2

what is the charge of the cation? FeSO4

Fe^2+

Identify ions in FeO

Fe^2+ and O^2-

Identify ions in Fe2O3

Fe^3+ and O^2-

gallium carbonate formula

Ga2(CO3)3

Write the chemical formula for ionic compound formed between: Selenium and gallium

Ga2Se3

Ga

Gallium

# of electrons lost by metal atoms =

Group #

Draw covalent bond for CH2O

H-C-H II O [O has 4 electrons around]

Draw covalent bond for C2H4

H-C=C-H I I H H

Draw covalent bond for C2H2

H-C[triple bond]C-H

Draw covalent bond for HCN

H-C[triple bond]N [N has 2 electrons around]

draw covalent bond for HCl

H-Cl [Cl has 6 electrons around]

Draw covalent bond for NH3

H-N-H I H [N has 2 electrons around]

Draw covalent bond for H2O

H-O-H [O has 4 electrons around]

what is the charge of the cation? TiPO4

Ti^3+

Name the compounds below: Sn(C2H3O2)2

Tin(II) acetate

Name the compounds below: Ti3N

Titanium(I) nitride

Why is an atom charge neutral?

Total # of protons = Total # of electrons

Total + charge =

Total - charge

Ionic Bond:

Transfer of electrons from one atom to another

Give chemical formulas for the compound below: Vanadium (III) carbonate

V2(CO3)3

Covalent bond model:

Valence shell of one physically overlaps valence shell of other. Now space around two nuclei is much larger for them to move in.

Ex: CuCl, CuCl2, Pb(C2H3O2)2, Pb(C2H3O2)4

Variable Charge Cations.

Example, Cl is chlorine

When it becomes monoatomic anion Cl^- it is chloride

Na: Z, P, e?

Z = 11, P= 11, e= 11

Give chemical formulas for the compound below: Zinc hydrogencarbonate

Zn(HCO3)2