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Chemistry Final Review

Total questions: 74

Worksheet time: 40mins

Name
Class
Date
1.

___ is the columns in the periodic table

a)

oxygen family

b)

group

c)

family

d)

period

2.

check all that applies for ions

a)

different # of electrons

b)

Same proton

c)

different #s of neutrons

d)

different number of proton

3.

Isotope has ...

a)

same protons, different electrons

b)

same protons, different neutrons

c)

different protons, same neutrons

d)

same protons, same neutrons

4.

cations are positive ions

a)

true

b)

false

5.

anions are positive ions

a)

true

b)

false

6.

Is Ca^2+ an anion or cation

a)

cation

b)

anion

7.

How many orbital does S sub level has

a)

7

b)

1

c)

3

d)

5

8.

How many orbital does P sub level have

a)

7

b)

1

c)

3

d)

5

9.

How many orbitals does Sub level D has?

a)

3

b)

1

c)

5

d)

7

10.

How many orbitals does F sub level has?

a)

7

b)

5

c)

3

d)

1

11.

what is the max number of electrons sub level S can have?

a)

2

b)

6

c)

10

d)

14

12.

what is the max number of electrons sub level P can have?

a)

6

b)

2

c)

10

d)

14

13.

what is the max number of electrons sub level D can have?

a)

14

b)

6

c)

2

d)

10

14.

what is the max number of electrons sub level F can have?

a)

2

b)

6

c)

14

d)

10

15.

which element is 1S^2 2S^2 2P^6 3S^2

a)

oxygen

b)

silicon

c)

magnesium

d)

Chlorine

16.

which element is shown?

a)

sulfur

b)

flourine

c)

oxygen

d)

neon

17.

the element shown is neon

a)

true

b)

false

18.

which is the correct noble gas configuration for Mg?

a)

(Ne) 3s^3

b)

[Ne] 3s^2

c)

[Ne] 2s^2

d)

(Ne) 3s^2

19.

what is the correct noble gas configuration of Sn? (Tin)

(a)  

20.

what is the correct noble gas configuration for Pb? (lead)

(a)  

21.

Aufbau's principle states ___?

a)

each electron must occupy lowest energy level first

b)

two arrows can occupy one orbital as long as they are pointing oppositly

c)

must occupy each orbital before moving on (empty bus seat)

22.

Hund's rule states ___?

a)

each electron must occupy lowest energy level first

b)

must occupy each orbital before moving on (empty bus seat)

c)

two arrows can occupy one orbital as long as they are pointing oppositly

23.

Pauli exclusion principal states ___?

a)

two arrows can occupy one orbital as long as they are pointing oppositly

b)

each electron must occupy lowest energy level first

c)

must occupy each orbital before moving on (empty bus seat)

24.

covalent bond

a)

exchange

b)

shares

25.

ionic bonds

a)

share

b)

exchange

26.

in a fireworks show, the fireworks explode giving off heat and light

a)

chemical change

b)

physical change

27.

food color is dropped in the water to give it color

a)

physical change

b)

chemical change

28.
a)

synthesis

b)

single replacement

c)

decomposition

d)

double replacemnt

29.
a)

synthesis

b)

decompostion

c)

single replacement

d)

double replacement

30.

what is the molar mass of CHCl3

a)

71.77 g/mol

b)

119.38 g/mol

c)

101.39g/mol

d)

56.12 g/mol

31.

How many grams of NO2 must react with H2O to produce 5.00x10^22 molecules of NO?

a)

11.5g H2O

b)

10.9g NO2

c)

11.5g NO2

d)

4.87x10^23

32.

what si constant in Boyles law

a)

all of the above

b)

temperature

c)

pressure

d)

volume

33.

what's constant in charles law

a)

pressure

b)

volume

c)

temperature

34.

what's constant in Gay Lussacs law?

a)

temperature

b)

volume

c)

pressure

35.

which law is the graph showing

a)

gay lussac

b)

boyle

c)

charles

36.

whos law does this equation belongs to

a)

charles

b)

gay lussacs

c)

boyle

37.

who's law is this showing

a)

charles

b)

gay lussac

c)

boyle

38.

If heat is shown in the reactant, it is showing__ reaction

a)

endothermic

b)

exothermic

39.

If the equation has negative heat, it is

a)

exothermic

b)

endothermic

40.

A reaction is __ if more energy is released than supplied

a)

exothermic

b)

endothermc

41.

Photosynthesis is an example of endothermic reaction

a)

true

b)

false

42.

dipole diple interaction is stronger than hydrogen bonding

a)

true

b)

false

43.

The idea that two electrons can occupy the same orbital because they have opposite spins.

a)

Pauli Exclusion Principle

b)

Aufbau Principle

c)

Hund's Rule

d)

The Electron Orbital Rule

44.

John Dalton

a)

First to theorize that all matter is made of atoms.

b)

Developed the Plum Pudding Model

c)

Believe that the atom was a solid sphere

d)

Used cathode rays and discovered electrons.

e)

discovered the neutron

45.

JJ Thomson

a)

First to theorize that all matter is made of atoms.

b)

Developed the Plum Pudding Model

c)

Believe that the atom was a solid sphere

d)

Used cathode rays which led to the discovery of electrons

e)

Discovered the neutron

46.

Rutherford

a)

First to theorize that all matter is made of atoms.

b)

Did the gold foil experiment

c)

Discovered the neutron and proton

d)

Used cathode rays which led to the discovery of electrons

e)

Discovered the nucleus and proton

47.

Bohr

a)

Made the Solar System Model

b)

Did the gold foil experiment

c)

Believed that electrons move around the nucleus and can have a certain # of electrons

d)

Used cathode rays which led to the discovery of electrons

e)

Discovered the neutron and proton

48.

Schrodinger

a)

Made the Solar System Model

b)

Did the gold foil experiment

c)

Believed that electrons move around the nucleus and can have a certain # of electrons

d)

Made the Electron Cloud Model

e)

Made an equation which found the position of electrons in an atom

49.

Chadwick

a)

Made the Solar System Model

b)

Discovered the neutron

c)

Believed that electrons move around the nucleus and can have a certain # of electrons

d)

Made the Electron Cloud Model

e)

Made an equation which found the position of electrons in an atom

50.

this is a picture of what

a)

test tube

b)

Erlenmeyer flask

c)

graduated cylinder

d)

beaker

51.

this is a picture of graduated cylinder

a)

false

b)

true

52.

who's model is the following shown?

a)

chadwick

b)

bohrdalton

c)

schrodinger

d)

bohr

53.

Q=mcΔT

How much energy is required to heat 120.0 g of water from 2 C to 24 C?

a)

4.184

b)

11045.76

c)

120

d)

11479.7

54.

Balance the equation

CH4 +Cl2 = CCl4 +HCl

a)

CH4 +4Cl2 = CCl4 +4HCl

b)

2CH4 +Cl2 = 2CCl4 +HCl

c)

CH4 +4Cl2 = CCl4 +2HCl

d)

2CH4 +2Cl2 = CCl4 +8HCl

55.

Is this equation balanced?

C12H22O11+ 8K(ClO3) =12CO2 + 11H2O+ 8KCl

a)

yes

b)

no

56.

what is the percent composition of C7H5 in the given equation

C7H5(NO2)3

a)

39%

b)

42%

c)

61%

d)

0.8%

57.

The image is showing what?

a)

freezing curve

b)

heating curve

c)

cooling curve

d)

boiling curve

58.

Two atoms which have large difference in electronegativity would form a(n)

a)

metalic bond

b)

ionic bond

c)

covalent bond

d)

polar and non-polar bond

59.

When you compare the atomic radius of Li vs Rb you would expect

a)

none has atomic radius

b)

Both has equal amount of atomic radius

c)

Li to have bigger atomic radius

d)

Rb to have bigger atomic radius

60.

in relation to the atom, the nucleus has the

a)

least mass and most volume

b)

least mass and least volume

c)

most mass and most volume

d)

most mass and least volume

61.

what is the molarity of the solution that contains 1.724 moles of H2SO4 in 2.5 L of solution?

a)

1.45 M

b)

0.68 M

c)

0.68 moles

d)

4.7 M

62.

Electronegativity increases as you move up and right.

a)

True

b)

False

63.

Atomic radius increases as you move up and to the left.

a)

True

b)

False

64.

How does metallic properties increase on the periodic table?

a)

Up and left

b)

down and right

c)

up and right

d)

down and left

65.

How does ionization energy increase along the periodic table?

a)

Up and left

b)

down and right

c)

up and right

d)

down and left

66.

On what principle does calorimetry depend?

a)

  Law of Conservation of Energy

b)

  Law of Enthalpy

c)

  Hess's Law

d)

  Law of Multiple Proportions

67.

How many grams of O2 are required to produce 358.5 grams of ZnO?

2Zn + O2 --> 2ZnO

a)

  29.1 g

b)

  1302 g

c)

  14.5 g

d)

  70.5 g

68.

The initial volume of a gas at a pressure of 3.2 atm is 2.9 L. What will the volume be if the pressure is increased to 4.0 atm?

a)

  2.5 atm

b)

  2.32 atm

c)

  4.41 atm

d)

  1.6 atm

69.

The Law of Conservation of Mass (or Matter) in a chemical reaction can be stated thus:

a)

  the products will be greater than the reactants

b)

  In a chemical reaction, matter is neither created nor destroyed.

c)

  energy is neither created or destroyed

d)

  the reactants will be greater than the products

70.

All atoms of the same element contain the same number of _______________.

a)

  protons

b)

neutrons

c)

electrons

d)

quarks

71.

The overall charge of an atom is ____________

a)

neutral

b)

positive

c)

negative

d)

  none of these

72.

Covalent Bonds

a)

The attraction between neutral atoms

b)

The attraction between positive atoms

c)

Shares electrons between two non-metals

d)

Exchanges electrons between a metal and a non-metal

e)

When electrons are shared equally

73.

Polar Covalent Bonds shares electrons equally and Non-Polar Covalent Bonds shares electrons unequally.

a)

True

b)

False

74.

Ionic Bonds

a)

The attraction between neutral atoms

b)

Usually cation and an anion

c)

Shares electrons between two non-metals

d)

Exchanges electrons between a metal and a non-metal

e)

When electrons are shared equally

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