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Semester 1 Final Revu

Total questions: 67

Worksheet time: 2hrs 41mins

Name
Class
Date
1.

Categorize the following characteristics of matter as either intensive or extensive.

Categorize the following

Color

Density

Boiling / Melting Point

Lustre

Malleability

Temperature

Mass

Volume

Length

Area

Moles

Intensive
Extensive
2.
The melting point of ice is 00 C. This is an example of ________.
a)
physical intensive property
b)
physical extensive property
c)
Chemical change
d)
Chemical property
3.
Wood burning is an example of _______
a)
physical intensive property
b)
physical extensive property
c)
chemical change
d)
Physical change
4.
Crumpling paper is an example of 
a)
physical change
b)
chemical change
c)
physical property
d)
chemical property
5.
The rose is red. This is an example of a 
a)
physical extensive property
b)
Chemical property
c)
physical intensive property
d)
physical change
6.
Which of the following is a chemical property of milk?
a)
it is white
b)
it has fats
c)
it has turns sour if left out of the refridgerator
d)
it is soluble in water
7.

​ ​ (a)   are dependent of the amount of substance present, such as mass, length, or volume

​ ​ ​

Choose from the below words
intensive properties
extensive properties
8.

​ ​ ​ (a)   are independent of the amount of substance present, such as density

​

Choose from the below words
intensive properties
extensive properties
9.

Toxicity - how poisonous something is

a)

chemical property

b)

intensive physical property

c)

extensive physical property

10.

Reactivity - the ability of a substance to cause a chemical reaction

a)

chemical property

b)

intensive physical property

c)

extensive physical property

11.

Classify the following a chemical or physical properties

Categorize the following

flammability

reactivity
pH level
oxidation state
density
color
hardness
luster
conductivity

toxicity

radioactivity

solubility (ability to dissolve in water)

physical
chemical
12.

A student mixes yellow powder with water. Which observation would prove a CHEMICAL change occurred?

a)

The powder DISSOLVED in the water

b)

The water turned the COLOR yellow

c)

The bag's TEMPERATURE changed

d)

The STATE OF MATTER changed

13.

What kind of change occurs if matter changes in amount, size, or shape?

a)

substance change

b)

chemical change

c)

physical change

d)

elemental change

14.
Physical properties are
a)
properties that can be observed without changing the identity of the substance
b)
properties that describe how a substance changes into a completely different substance
15.

What is a chemical change?

a)

Forming a new substance

b)

When two or more substances combine to make a greater one

c)

When two or more substances combine to make a new chemical substance

d)

Combing substances

16.
Which of the following is not a chemical property? 
a)
rusting 
b)
boiling 
c)
rotting 
d)
burning 
17.

Chemical or Physical Change?

Categorize the following
Chemical
Physical
18.

Which of the following elements has the largest atomic radius?

a)

oxygen

b)

sulfur

c)

phosphorus

d)

nitrogen

19.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

20.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
21.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
22.

Which element has 3 valence electrons?

a)

A

b)

B

c)

E

d)

C

23.
Which elements have the same number of valence electrons?
a)
A & C
b)
E & C
c)
F & A
d)
F & B
24.
List the two most reactive families on the periodic table.
a)
Alkali metals & Transition Metals
b)
Noble gases & Oxygen Family
c)
Halogens & Alkali metals
d)
Halogens & Noble gases
25.

The tendency of an atom to attract a shared pair of electrons

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

26.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
27.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)

oxygen (O)

28.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
29.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)

the number of protons increases, causing electrons to be more attracted to the nucleus

b)
the number of energy levels increases
c)

the number of electrons increases, causing the electron cloud to expand

d)
the atomic mass increases
30.

What is the strength of an atom's pull on electrons in a bond called?

a)

atomic radius

b)

ionization energy

c)

electronegativity

31.

How many full inner shells are beneath the outer valence electron shell of Calcium (Ca)?

a)

1

b)

2

c)

3

d)

4

32.

Which of the following have a luster, are malleable, are ductile, and are good conductors of heat and electricity?

a)

metals

b)

nonmetals

33.

Which outline of elements are known as the transition metals?

a)

A

b)

B

c)

C

d)

D

34.

What does Nitrogen (N) want to do to obtain a full outer valence shell?

a)

gain 2 electrons

b)

gain 3 electrons

c)

lose 2 electrons

d)

lose 3 electrons

35.

Which element is the most electronegative element on the periodic table?

a)

Oxygen (O)

b)

Fluorine (F)

c)

Sulfur (S)

d)

Chlorine (Cl)

36.

An atom of ____ could be represented by the Lewis dot diagram shown above.

a)

Mg

b)

Cl

c)

C

d)

O

37.

Atomic radius is defined as ____.

a)

the relative size of the atom's nucleus

b)

the relative size of the atom's electron cloud

c)

the energy required to shield the outer electrons from the nucleus

d)

a measure of the ability of an atom to attract electrons

38.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
39.

Ionic Bonding is the _________ of electron/s between atoms.

a)

sharing

b)

transfer

c)

loose

d)

gain

40.

Electron that is located on the outermost shell

a)

proton

b)

neutron

c)

electron

d)

valence electron

41.

A bond between metal and non metal is called

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

42.

If an atom loses two electrons what charge will it have?

a)

-1

b)

-2

c)

+1

d)

+2

43.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
44.
If atoms that are sharing electrons have an unequal attraction for the electrons it is a ____
a)
Ionic bond
b)
Nonpolar covalent bond
c)
Polar covalent bond
d)
Metallic bond
45.
Which of these molecules has nonpolar covalent bonding?
a)
H2O
b)
HCl
c)
I2
d)
NaCl
46.
When forming an ionic bond, a metal atom
a)
Gains electrons to form a cation
b)
Loses electrons to form a cation
c)
Gains electrons to form an anion
d)
Loses electrons to form an anion
47.
Metals form ions by _____________ electrons, nonmetals form ions by   ___________ electrons. 
a)
losing, gaining
b)
gaining, losing
c)
 losing, losing
d)
gaining, gaining
48.

What type of bonding is present in dinitrogen pentoxide, N2O5?

a)

ionic

b)

covalent

c)

metallic

d)

bionic

49.

In metallic bonds, the force of attraction is between

a)

positive and negative ions

b)

cations and electrons

c)

two different metals

d)

neutrons and electrons

50.

Metals are used to make electric wires because metals (choose all that apply)

a)

are ductile

b)

are shiny

c)

have free moving electrons

d)

form a lattice

51.

How does a metallic lattice differ from an ionic crystal?

a)

A metallic lattice is less flexible

b)

A metallic lattice can change shape without breaking

c)

A metallic lattice shatters when struck

52.

There are 3 substances on the table. Substance A is a white powder with a high melting point and conducts in a solution. Substance B is a silver gray solid with a high melting point. Substance C is a white solid with a low melting point that doesn't conduct. Based on the properties, what are the bonds of each material.

a)

A has covalent bonds, B has ionic bonds, and C has metallic bonds

b)

B has covalent bonds, C has ionic bonds, and A has metallic bonds

c)

C has covalent bonds, A has ionic bonds, and B has metallic bonds

d)

Not enough information

53.

What type of bond is NaF

a)

Ionic

b)

Covalent

c)

Metal

d)

No bond can form

54.

Which is of the following is NOT true about ionic compounds?

a)

Ionic compounds are brittle

b)

Ionic compounds melt easily

c)

Ionic compounds conduct electricity in water

d)

Ionic compounds are made of positive and negative ions

55.

Ionic compounds have _________ electronegativity difference

a)

large

b)

small

c)

what is electronegativity?

d)

medium

56.

How do particles in a solid move?

a)

they slide past each other

b)

they vibrate in place

c)

they don't move at all

d)

they move freely and rapidly

57.

Matter that has a fixed volume but no fixed shape is…

a)

solid

b)

liquid

c)

gas

d)

plasma

58.

What is the name of the phase change from gas to liquid?

a)

freezing

b)

deposition

c)

vaporization

d)

condensation

59.

What is the name of the phase change from liquid to solid?

a)

freezing

b)

deposition

c)

vaporization

d)

condensation

60.

Matter in which the particles are free to move in all directions until they have spread evenly throughout their container is a...

a)

plasma

b)

liquid

c)

gas

d)

solid

61.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
62.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
63.
Identify this atom: 
a)
Lithium
b)
Chlorine
c)
Phosphorus 
d)
Fluorine
64.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
65.

What electron configuration matches an Bromine?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

66.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
67.

Label the 3 states of matter shown here

a)

Solid

b)

Liquid

c)

Gas

1
2
3
1)
2)
3)

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