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Chem Ch. 3 and 6 Elements, Periodic Table, Acids, Bases, pH

Total questions: 67

Worksheet time: 1hrs 7mins

Name
Class
Date
1.

All matter is made of

a)

energy

b)

atoms

c)

electrons

d)

compounds

2.
Two atoms of the same element but with different mass numbers are called________
a)
electrons
b)
isotopes
c)
variables
d)
electron cloud
3.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
4.

The horizontal rows on the periodic table are called:

a)

Shells

b)

Periods

c)

Groups

d)

Horizontals

5.

The vertical columns on the periodic table that have common properties are called

a)

Groups

b)

Periods

c)

Shells

d)

Valences

6.

The Russian scientist who created one of the first periodic tables by using atomic mass was:

a)

Bohr

b)

Rutherford

c)

Mendeleev

d)

Thomson

7.

What do atoms of the same periodic group have in common?

a)

They have the same atomic number.

b)

They have the same chemical symbols.

c)

The have similar chemical properties.

d)

They have the same atomic mass.

8.
John was observing the physical properties of elements in order to classify them as either a metal, nonmetal, or metalloid. The first element was dull, brittle, and did not conduct heat. What would its classification be? 
a)
metal 
b)
nonmetal 
c)
metalloid
9.

The ______ are usually shown below the main portion of the periodic table.

a)

Actinides and lanthanides

b)

Metalloids and noble gases

c)

valence electrons

10.

This group on the periodic table is all made in a lab.

a)

Actinides and lanthanides

b)

Alkali earth metals

c)

Halogens

d)

Transition metals

11.

Mendeleev's periodic table arranged elements by

a)

atomic number.

b)

atomic mass.

c)

number of neutrons.

d)

electronegativity.

12.

Elements with atomic numbers greater than that of uranium are called ____________ elements.

a)

suburanium

b)

hyperuranium

c)

transuranium

d)

posturanium

13.

The most commonly used metals are transition metals.

a)

true

b)

false

14.

Which scientist came up with the Atomic theory and said that atoms were like smooth, round balls?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

15.

Which characteristics does NOT describe an acid?

a)

tastes sour

b)

reacts with metal

c)

feels slippery

d)

corrosive

16.

Which of the following is an acid?

a)

soap

b)

baking soda

c)

orange juice

d)

water

17.

Which of the following is a base?

a)

carbonated water

b)

lime juice

c)

vinegar

d)

dishwashing detergent

18.

The pH scale is a range from

a)

1 to 7

b)

7 to 14

c)

1 to 14

d)

1 to 20

19.

A very strong acid would have a pH of

a)

1

b)

7

c)

9

d)

14

20.

Which chemical produces OH- ions when mixed with water?

a)

Acid

b)

Base

21.

Acid mixed with a base will __________ the mixture.

a)

nullify

b)

neutralize

c)

balance

d)

naturalize

22.

Which pH number below reflects a weak acid?

a)

1

b)

6

c)

8

d)

13

23.

Which pH number below reflects a weak base?

a)

1

b)

6

c)

8

d)

13

24.

Which pH number below reflects a strong base?

a)

1

b)

6

c)

8

d)

13

25.

Which chemical makes red litmus paper turn blue?

a)

Acid

b)

Base

26.

Which chemical makes blue litmus paper turn red?

a)

Acid

b)

Base

27.

Which characteristics does NOT describe an base?

a)

tastes sour

b)

slippery feel

c)

tastes bitter

d)

turns red litmus paper blue

28.

Which chemical produces H+ ions when mixed with water?

a)

Acid

b)

Base

29.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

30.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
31.

These are found in the nucleus and have a neutral charge.

a)

proton

b)

electron

c)

neutron

32.

In an atom, the number of protons is equal to the number of ____________.

a)

energy levels

b)

neutrons

c)

neurons

d)

electrons

33.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
34.

How many electrons does an Iodine atom have?

a)

53

b)

126

c)

73

d)

179

35.

How many neutrons does an Oxygen atom have?

a)

8

b)

16

c)

24

d)

7.999

36.
What is atomic number?
a)
Number of protons in an atoms 
b)
Number of neutrons in an atom
c)
Mass of an atom
d)
Charge on an atom
37.
Which subatomic particles are found in the nucleus of an atom?
a)
Protons and Electrons
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons, Neutrons and Electrons
38.
The total number of protons and neutrons in an atom is called the...
a)
Atomic number
b)
Proton number
c)
Mass number
d)
Weight number
39.

This model has negatively charged particles mixed throughout a positive "soup". We have also called it the chocolate chip cookie or watermelon model

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

40.

The atom was made up of mostly empty space with a dense positively charged nucleus and negative charges outside

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

41.

This model of the atom is also called the shows electrons orbiting the nucleus in distinct energy levels

a)

Dalton

b)

Thomas

c)

Rutherford

d)

Bohr

42.

This is a type of mixture where one substance dissolves into another

a)

Solution

b)

Miscibility

c)

Compound

d)

Solubility

43.

Which is an example of a solution?

a)

Salt and Sugar

b)

Salt Water

c)

Jelly beans

d)

Concrete

44.
What type of mixture separates upon standing?
a)
Solution
b)
Alloy
c)
Colloid
d)
Suspension
45.
What is the solvent in a solution of kool-aid and water?
a)
glass
b)
kool-aid
c)
water
46.
___________ is a combination of substances that can be physically separated. 
a)
Colloid 
b)
Mixture 
c)
Suspension 
d)
Compound 
47.
A mixture can be classified as a solution, suspension or colloid based on the 
a)
number of particles it contains
b)
size of its largest particles
c)
color of its particles
d)
size of its smallest particles
48.
type of mixture that doesn't separate on its own but still contains undissolved particles
a)
solution
b)
colloid
c)
suspension
49.

The substance being dissolved is called the ________

a)

solvent

b)

solid

c)

solute

d)

solvate

50.

a substance in which another substance is dissolved

a)

Solute

b)

Product

c)

Reactant

d)

Solvent

51.

Water is the universal ____.

a)

solute

b)

solvent

c)

solution

52.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

53.

What pH does a neutral substance have?

a)

5

b)

6

c)

7

d)

8

54.
As you move from left to right across the periodic table, the atomic number increases. 
a)
True
b)
False
55.

Which elements are shiny (lustrous) and malleable?

a)

Metals

b)

Nonmetals

c)

Metalloids

56.

Which elements are good conductors of electricity and heat?

a)

Metals

b)

Nonmetals

c)

Metalloids

57.

Which of the following is the most reactive group of metals?

a)

Alkali

b)

Alkaline Earth

c)

Halogen

58.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
59.

Which of the following groups is nonreactive and will not form bonds with any other element?

a)

Alkali

b)

Transition Metals

c)

Noble Gas

d)

Halogens

60.

The elements in this family are soft, silvery, and very reactive with water.

a)

Alkaline Earth Metals

b)

Alkali Metals

c)

Transition Metals

d)

Lanthanides

61.

Label the parts of the atom

a)Proton
b)Electron
c)Neutron
1
2
3
1)
2)
3)
62.

Solution___ is the most concentrated

a)

1

b)

2

c)

3

d)

4

63.
The maximum amount of a solute that can be dissolved in a given amount of solvent at a given temperature.
a)
solubility
b)
concentrated
c)
diluted
d)
surface area
64.
A solution that can hold more solute  is called
a)
saturated
b)
supersaturated
c)
unsaturated
d)
insoluble
65.

When a solution cannot dissolve more solute, it is called

a)

saturated

b)

supersaturated

c)

unsaturated

d)

solvent

66.

Which of the following would increase the amount of solute dissolved?

a)

decreasing temperature

b)

increasing temperature

c)

decreasing amount of solvent

d)

increasing amount of solute

67.

Which substance is least soluble at 0 ºC?

a)

KI

b)

KNO3

c)

KClO3

d)

Ce2(SO4)3

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