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FINAL EXAM REVIEW

Total questions: 146

Worksheet time: 4hrs 26mins

Name
Class
Date
1.

Al + H2SO4 ->

How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?

a)

0.85 g

b)

290 g

c)

450 g

d)

870 g

2.

Cl2 + KBr →

how many grams of potassium chloride can be produced from 356 grams potassium bromide?

a)

749 g

b)

223 g

c)

479 g

d)

814 g

3.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
4.

LiOH + KCl →

I actually produced 6 grams of lithium chloride and I began this reaction with 20 grams of lithium hydroxide. What is my percent yield?

a)

16.9%

b)

5.91%

c)

1.88%

d)

12.3%

5.

CH4 + 2O2 → CO2 + 2H2O

24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.

a)

66 grams

b)

132 grams

c)

33 grams

d)

8.72

6.

2Fe2O3 + C → Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.8%

b)

308%

c)

6435%

d)

15.5

7.

P4 + 6Cl2 --> 4PCl3

The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction.

a)

78%

b)

64%

c)

27%

d)

33%

8.

2Pb(NO3)2 (s)→2PbO(s)+4NO2(g)+O2(g)

Lead nitrate can be decomposed by heating. What is the % yield of the decomposition reaction if 7.4g Pb(NO3)2 are heated to give 4.1 g PbO?

a)

82%

b)

44%

c)

56%

d)

67%

9.

Zn + HCl → ​​

15 grams of HCl should theoretically produce 0.41 grams of H2. The reaction actually produced 0.15 grams of H2. What is the percent yield of H2?

a)

2.8%

b)

280%

c)

1%

d)

37%

10.

An ionic compound forms between a _______ and _______.

a)

metal and non-metal

b)

two metals

c)

two non-metals

11.

Name the ionic compound, LiCl

a)

lithium chlorine

b)

lithium chloride

c)

lithium chlorate

d)

lithium monochloride

12.

Name the ionic compound, FeBr3

a)

Iron (II) bromide

b)

Iron (III) bromide

13.

What is the formula for diphosphorus pentoxide?

a)

P2O5

b)

PO5

c)

P5O2

d)

Po2O5

14.

What is the name for SiCl4?

a)

silicon tetrachloride

b)

silicon quadchloride

c)

monosilicon tetrachloride

d)

silicon chloride

15.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

lead + oxygen

16.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

17.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

18.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide
19.
H2SO4 - name?
a)
hydrogen sulfide
b)
hydrosulfuric acid
c)
hydrogen sulfide
d)
sulfuric acid
20.

The following properties are all characteristics of ionic compounds EXCEPT

a)

solid at room temperature

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

21.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

A firm handshake

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

22.

Which type of bond is formed from the sharing of electrons?

a)

ionic bond

b)

covalent bond

23.

What set of elements is most likely to form a covalent compound?

a)

Na and O

b)

Na and K

c)

O and C

24.

Which set of elements is most likely to form an ionic compound?

a)

Na and O

b)

C and O

c)

Na and K

25.

The bond between C and Cl is polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

26.

The bond between C and H is non-polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

27.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

28.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

29.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

30.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

31.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
32.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

33.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
34.

You are given 40.05g S and 59.95g O. Find the empirical formula for these elements.

a)

SO

b)

SO2

c)

SO3

d)

SO4

35.

A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?

a)

Mg4N3

b)

MgN2

c)

Mg3N2

d)

MgN

36.

What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.

a)

K2SO4

b)

K8SO16

c)

K8S4O8

d)

K8S4O16

37.

What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?

a)

CH2O

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

38.

Na2CO3 · 10H2O is known as sodium carbonate ______

a)
Hydroxide
b)
Hydrate
c)
Decahydrate
d)
None of the above
39.
Name the following hydrate:  NaCl * 5H2O
a)
sodium chloride 
b)
sodium monochloride pentahydrate
c)
sodium chloride pentahydrate
d)
pentahydrate
40.
A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
a)
MgCO3 · 5H2O
b)
MgCO3 · 4H2O
c)
MgCO3 · 6H2O
d)
MgCO3 · 1H2O
41.

A 4.175 gram sample of a certain hydrate of copper (II) sulfate, CuSO4•xH2O, is heated until all the water is driven off. The resulting anhydrous compound weighs 3.120 grams. What is the formula of the hydrate?

a)

CuSO4•H2O

b)

CuSO4•3H2O

c)

CuSO4•6H2O

d)

CuSO4•4H2O

42.
4Si + S8 --> 2Si2S4
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Double displacement
43.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single diplacement
d)
Double displacement
44.
2Pb(NO3)2 --> 2PbO + 4NO2 + O2
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Combustion
45.
Which reaction type is the following: C5H10O4 + O2 --> CO2 + H2O
a)
Decomposition
b)
Single Replacement
c)
Combustion
d)
Double Replacement
46.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
47.
Balance this equation:
 __Li + __Cl2 -> __LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li +  Cl2 -> 2LiCl
48.
PbCl2 + AgNO3 ---> Pb(NO3)2 + AgCl 
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
49.

If an element is diatomic it should have a subscript of___

a)

1, always

b)

2, only when it is an element

c)

it shouldn't have a subscript, it should have a coefficent

d)

2, when bonded in a compound

50.

What is the charge of Iron in this compound. (Hint: think swap drop method):

Fe3(PO4)2

a)

3+

b)

2+

c)

1+

d)

6+

51.

The symbol for a substance dissolved in solution is ______

a)

(s)

b)

(l)

c)

(aq)

d)

(g)

52.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

53.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

54.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

55.

Complete the balanced equation for this Double Replacement reaction.

3 NaOH + Fe(NO3)3 →

a)

NaFe + OH(NO3)3

b)

NaNO3 + Fe(OH)3

c)

3 NaNO3 + Fe(OH)3

d)

3 NaFe + 3 (OH)NO3

56.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

57.

What are the products of this reaction:

C2H4 + O2 →

a)

C2O2 + H4

b)

CO2 + H2 + O2

c)

CO + H

d)

CO2 + H2O

58.

Predict the products of this single replacement reaction: Na + H2O →

a)

NaO + H2

b)

NaOH + H2

c)

NaH + O2

d)

ONaH

59.
Based on the activity series, will this reaction occur?
Ni (s) + H2O (l) →
a)
Yes
b)
No
60.
Based on the activity series, will this reaction occur?
Br2 (l) + KI (aq) →
a)
Yes
b)
No
61.
Based on the activity series, will this reaction occur?
Au (s) + HCl (l) →
a)
Yes
b)
No
62.

Predict the product(s) of this reaction (don't worry about balancing):

Li + H2O →

a)

Li2O + H2

b)

LiO + H2

c)

LiOH + H2

d)

Li(OH)2

63.

Based on the activity series, which metal could X represent in the reaction below?

X + Ca (NO3)2 --> Ca + X (NO3)2

a)

Ba

b)

Fe

c)

Mg

d)

Zn

64.

Soluble or insoluble? Mg(NO3)2

a)

soluble

b)

insoluble

65.

Soluble or insoluble? BaSO4

a)

soluble

b)

insoluble

66.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)

2Ag+(aq)  +  2Cl- (aq) → 2AgCl(s)

c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
67.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
68.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
69.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
70.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
71.

3NH4NO3 + Na3PO4 --> (NH4)3PO4 + 3 NaNO3


Assuming we start with 30 g of NH4NO3 and 50 g of Na3PO4, identify the limiting reactant.

a)

ammonium phosphate

b)

sodium phosphate

c)

ammonium nitrate

d)

sodium nitrate

72.

3NH4NO3 + Na3PO4 --> (NH4)3PO4 + 3 NaNO3

Assuming we start with 30 g of NH4NO3 and 50 g of Na3PO4, What is the maximum amount of each product that can be formed?

a)

18.6 g of ammonium phosphate, 31.9 of sodium nitrate

b)

54 g of ammonium phosphate, 31.9 of sodium nitrate

c)

32.4 g of ammonium nitrate, 76 g of sodium phosphate

d)

21 g of ammonium nitrate, 34 g of sodium phosphate

73.
Name the following hydrate:  NaCl * 5H2O
a)
sodium chloride 
b)
sodium monochloride pentahydrate
c)
sodium chloride pentahydrate
d)
pentahydrate
74.

Which of the following is an empirical formula? 

a)

CH2O

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

75.

A 3.11 g sample of ZnSO4 ⋅ 7H2O is heated to dryness. Determine the mass of anhydrous salt remaining after all the water has been driven off.

a)

3.11 g

b)

1.75 g

c)

1.36 g

d)

0.562 g

76.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

77.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
78.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
79.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
80.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
81.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
82.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
83.

What is the correct shape of CHCl3?

a)

Bent

b)

Trigonal pyramidal

c)

Tetrahedral

d)

Trigonal planar

84.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
85.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
86.

What molecule could this be? (Each purple cloud represents a lone pair of electrons.)

a)

CO2

b)

NH3

c)

H2S

d)

CH4

87.

What molecule could this be? (The purple cloud represents a lone pair of electrons.)

a)

H2O

b)

NH3

c)

CO2

d)

CH4

88.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
89.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
90.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
91.

This is what you call a reactant that you have enough of. The one that DOES NOT run out.

a)

Limiting Reactant

b)

Excess Reactant

c)

Highly Reactant

d)

Super Reactant

92.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
93.

P4 + 3O2 --> P4O6

How many moles of P4O6 can be made if 3 moles of P4 react with 6 moles of O2?

a)

1 mole

b)

2 moles

c)

4 moles

d)

0 moles

94.
What are the products of this reaction?
Cu+ AgNO3--> 
a)
Cu(NO3)2+Ag
b)
CuNO3 + Ag
c)
CuAg+NO3
d)
Cu+ AgNO3
95.
Predict the products for the this reaction:
K + HCl --> 
a)
KCl + H2
b)
KHCl 
c)
KH + Cl2
d)
KCl + H
96.
Which of the following equations represents the balanced synthesis reaction of iron (III) and oxygen?
a)
Fe + 3 O2 → Fe2O3
b)
3 Fe + 3 O2 → 2 Fe2O3
c)
2 Fe + O2 → Fe2O3
d)
4 Fe + 3 O2 → 2 Fe2O3
97.
What kind of reaction is this:
4Fe  +  3O2 →   2Fe2O3 
a)
Synthesis
b)
Decomposition
c)
Single Replacement 
d)
Double Replacement
98.
What kind of reaction is this:
2H2O2 →2 H2O + O2
a)
Synthesis
b)
Decomposition
c)
Single Replacement 
d)
Combustion
99.
Based on the activity series, will this reaction occur?
Ni (s) + H2O (l) →
a)
Yes
b)
No
100.
Based on the activity series, will this reaction occur?
Br2 (l) + KI (aq) →
a)
Yes
b)
No
101.
Based on the activity series, will this reaction occur?
Au (s) + HCl (l) →
a)
Yes
b)
No
102.

Predict the product(s) of this reaction (don't worry about balancing):

Li + H2O →

a)

Li2O + H2

b)

LiO + H2

c)

LiOH + H2

d)

Li(OH)2

103.
What  will be the result of the following: 
Br2 + NaF ->
a)
bromine will replace Na
b)
Na will replace Br
c)
Br will replace F
d)
no reaction will occur
104.
What  will be the result of the following: 
Li + NaF ->
a)
Li will replace F
b)
Na will replace Li
c)
Li will replace Na
d)
no reaction will occur
105.
What  will be the result of the following: 
LiBr + Na ->
a)
Li will replace Na
b)
Na will replace Br
c)
Na will replace Li
d)
no reaction will occur
106.
KBr
a)
Soluble
b)
Insoluble
107.
Silver Iodide
a)
Soluble 
b)
Insoluble 
108.
KOH
a)
Soluble 
b)
Insoluble
109.
PbI2
a)
Soluble
b)
Insoluble
110.
NaC2H3O2
a)
soluble
b)
insoluble
111.
CaCO3
a)
soluble
b)
insoluble
112.
BaSO4
a)
soluble
b)
insoluble
113.
NH4NO3
a)
soluble
b)
insoluble
114.

What of these is always soluble?

a)

Nitrates

b)

Phosphates

c)

Carbonates

d)

Hydroxides

115.

What is the state of matter symbol for a soluble compound?

a)

(s)

b)

(aq)

c)

(g)

d)

(l)

116.
What is the state of matter symbol for an insoluble compound?
a)

(s)

b)

(aq)

c)

(g)

d)

(l)

117.

Predict the products of this reaction: Al2(SO4)3 + Ca3(PO4)2 --->

a)

This reaction will not occur

b)

Al(PO4) + Ca(SO4)

c)

Al2Ca3 + (PO4)2(SO4)3

d)

Al2(SO4)3 + Ca3(SO4)3

118.

Predict the products of this reaction: AgF + KCl --->

a)

This reaction will not occur.

b)

AgCl + KF

c)

AgCl3 + KF2

d)

AgK + ClF

119.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
120.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
121.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
122.

The products for FeCl3 + AgNO3 ----> are...

a)

Fe(NO3)3 (aq) + AgCl (s)

b)

FeNO3 (aq) + AgCl3 (s)

c)

Fe(NO3)3 (s) + AgCl (aq)

123.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
124.

The name for the chemical formula AlCl3

a)

aluminum chlorine

b)

aluminide chloride

c)

aluminum trichloride

d)

aluminum chloride

125.
Which of the following is an ionic compound?
a)
CCl4
b)
CO2
c)
NO2
d)
CuCl2
126.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
127.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
128.

When balancing an equation you can only add or adjust:

a)

coefficients

b)

subscripts

c)

parentheses

d)

exponents

129.
Cations are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
130.

What is the noble gas configuration for oxygen?

a)

[Ar] 3p⁴

b)

[He] 3s² 3p⁴

c)

[He] 2s² 2p⁴

d)

[Li] 2s² 2p⁴

131.

What happens to the energy of an electron as it moves from n=4 to n=2?

a)

energy is absorbed

b)

energy is released

c)

energy remains the same

d)

unable to determine

132.

What is the percent composition of oxygen in BaCrO₄?

a)

20.5%

b)

25.3%

c)

54.2%

d)

9.5%

133.

How many moles of silver atoms are in 1.8 x 10²⁴ atoms of silver?

a)

3.0 x 10¹ mol

b)

3.0 x 10⁻¹ mol

c)

3.0 mol

d)

1.1 x 10⁴⁴ mol

134.

1 mole of helium gas occupies what volume at STP?

a)

22.4 L

b)

0 °C

c)

1 atm

d)

4.00 L/mol

135.
Which element is a metalloid?
a)
Na
b)
N
c)
Ge
d)
K
136.

How many molecules are in 2.5 mol of NaCl?

a)

1.51x1023

b)

146

c)

4.15

d)

1.51x1024

137.
What is the molar mass of (NH4)2O?
a)
34 g/mol
b)
33 g/mol
c)
49 g/mol
d)
50 g/mol
138.
Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a)
double replacement 
b)
decomposition 
c)
combustion 
d)
single replacement
139.

When Ryan poured vinegar on baking soda, which of the following was a sign that a chemical change occurred?

a)

nothing happened

b)

it fizzed and produced gas

c)

it glowed

d)

its color became darker

140.

Protons have a ____________ charge.

a)

Positive

b)

Negative

c)

Neutral

141.

Neutrons are found ____________ the nucleus.

a)

Inside

b)

Outside

142.

The number of protons in an atom. It is the same as the number of electrons.

a)

Atomic Mass

b)

Atomic Number

c)

Element

d)

Compound

143.

The columns in the periodic table.

All members of groups/families behave the same way; they have the same chemical properties.

a)

Groups/Families

b)

Periods

144.

Shiny, good conductors of heat, usually solid at room temperature, able to be molded into shapes.

Example: Lithium, Sodium, Magnesium, Calcium

a)

Metals

b)

Nonmetals

145.

The most reactive metals in the table.

React best with Group 17 of the nonmetals.

Example: Hydrogen, lithium, sodium, potassium, rubidium, cesium, francium.

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

146.

Matter that is different throughout, the parts of the mixture are distinguishable.

Example: Chex mix, chocolate chip cookie, sandwich, salad, pizza

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

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