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
