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Ch. 2 Chem Review for BIO

Total questions: 60

Worksheet time: 49mins

Name
Class
Date
1.

All matter is made of what?

a)

energy

b)

atoms

c)

electrons

2.

The positive particles of an atom are ___________.

a)

electrons

b)

protons

c)

neutrons

3.

The center of an atom where its neutrons and protons are is called the _____________.

a)

nucleus

b)

electron cloud

c)

center

4.

An atom with atomic number 6 would have how many protons?

a)

6

b)

12

c)

3

d)

5

5.

Particles in an atom that are neutral and have no charge are

a)

protons

b)

electrons

c)

neutrons

6.

What is the atomic number for an element with three protons and 4 neutrons?

a)

6

b)

4

c)

3

d)

7

7.

This energetic particle with negligible mass and a negative charge, moves around the nucleus.

a)

Proton

b)

Neutron

c)

Electron

d)

Quark

8.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
9.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)

mass number

10.
What is the number of protons that the element in this image contain?
a)

16

b)

31

c)
15
d)

30

11.

What is the number of neutrons that the element in this image contain?

a)

16

b)

31

c)
15
d)

30

12.

What is the most common mass number for Iodine?

a)

53

b)

74

c)

126.904

d)

127

13.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
14.

Different isotopes of the same element have...

a)

different masses

b)

different number of protons

c)

different number of electrons

d)

different number of neutrons

e)

different number of neutrons and electrons

15.

The stability of a nucleus depends on the balance between these two opposing forces in an atom?

a)

strong force

b)

electronic force

c)

Coulombic force

d)

Intermolecular force

e)

intramolecular force

16.

The atomic mass (weight) represents the weighted average of the ________ of an element.

a)

electrons

b)

isotopes

c)

protons

d)

isomers

17.
How is carbon-12 different from carbon-14?
a)
They have a different number of protons 
b)
They have a different number of electrons
c)
They have a different number of neutrons
d)
They are different elements 
18.

This particle determines which element you have.

a)

electron

b)

proton

c)

neutron

d)

valence shell

19.

What is the approximate mass of a proton or a neutron?

a)

1 amu

b)

2 X 10 23 g

c)

1 g

d)

0.0005 amu

20.
What is the mass number and name of an element with 8 protons and 8 neutrons?
a)
16 - Carbon
b)
16 - Oxygen
c)
24 - Oxygen
d)
8 - Neon
21.
The mass of one proton is equal to the mass of one...
a)
neutron
b)
electron
c)

quark

d)

1/2000 the mass of an electron

22.

Nearly all of the mass of an atom comes from what location?

a)

nucleus

b)

electron cloud

c)

neutrons only

d)

protons only

23.

What is the volume of an atom mostly composed of?

a)

protons

b)

the nucleus where protons and neutrons are found

c)

empty space where electrons are likely to be found

d)
neutrons
24.

How does the size of an electron compare to a proton?

a)

electrons are about 2000 times larger than a proton so they make up most of the mass of atoms

b)

electrons are about 1800 times smaller so we consider them insignificant to the overall mass of the atom

c)

electrons are nearly the same size as a proton

d)

electrons have no size

25.

The reactivity or chemical properties of an atom are determined by

a)

protons

b)

neutrons

c)

electrons

d)

protons & neutrons

26.

The force between neutrons and protons in the nucleus that holds the nucleus together is called

a)

Coulombic force

b)

Stable force

c)

Strong force

d)

Cool Force

27.

Atoms with unstable nuclei are ...

a)

always very dangerous

b)

noble gases

c)

extra reactive

d)

radioactive

28.

Put the following elements in order from lowest to highest abundance (by mass) in the human body.

a)

O

b)

C

c)

H

d)

N

e)

Ca

1)
2)
3)
4)
5)
29.

When do ionic compounds conduct electricity

a)

when solid

b)

when molten

c)

when dissolved

d)

when in a plasma state

30.

Which of the following is not a property of a covalent compound?

a)

particles are called formula units

b)

can be solid, liquid or gas at room temp

c)

poor conductor of electricity

d)

may or may not dissolve in water

31.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

32.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
33.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

an attraction between 2 or more metals

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

34.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
35.
A covalent bond is
a)
a bond that shares electrons metallicaly
b)
A bond that shares electrons with non metals
c)
Metalloids bonding
d)
metals and nonmetals bonding
36.

How are atoms held together in covalent bonds?

a)

By gaining electrons

b)

By sharing electrons

c)

By losing electrons

d)

By transferring electrons

37.

In forming covalent bonds, why do atoms share electrons?

a)

To achieve noble-gas electron configuration

b)

To become charged

c)

To form ions

d)

To empty electron shells

38.

In a polar covalent bond, electrons are shared ____________ between two atoms.

a)

equally

b)

unequally

c)

closely

39.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

40.
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
41.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that attracts electrons less

b)

The atom with the greater electronegitivity

c)

The atom that attracts more electrons

d)

The atom with the lower electronegativity

42.

Which of the following types of compounds will likely dissolve in water, since water is polar?

a)

ionic compounds

b)

polar or hydrophilic molecules

c)

nonpolar or hydrophobic molecules

d)

metallic compounds

43.
Does H2O have hydrogen bonding?
a)
yes
b)
no
44.

What explains the relatively high melting and boiling point of water (higher than some covalent compounds as it is not a gas at room temp)?

a)

weak dipole forces between water molecules

b)
Hydrogen bonds between water molecules
c)

lack of polarity in water

d)
Molecule-ion attractions between water molecules
45.
Which type of solid is hard, brittle, and nonconducting unless dissolved in H2O?
a)
Ionic Crystal
b)
Covalent Molecular Crystal
c)
Metallic Crystal
d)
Covalent Network Crystal
46.

A polar covalent bond is an example of an ____________ force while a hydrogen bond is an example of ________________ force.

a)

intermolecular/intramolecular

b)

intermolecular/intermolecular

c)

intramolecular/ionic

d)

intramolecular/intermolecular

47.

DNA strands are held together by these bonds that occur between the nitrogen bases on each strand due to the fact that N - H bonds present.

a)

dipole-dipole forces

b)

London dispersion forces

c)

H-bonds

d)

ionic forces

48.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
49.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
50.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
51.

Which of the following could make a good electrolyte?

a)
sodium chloride
b)

table sugar

c)
water
d)

olive oil

52.
Solutions in which electric currents cannot run through are said to be
a)
noncolloidal
b)
electrolytes
c)
nonelectrolytes
d)
conductors
53.
An example of a nonelectrolyte is
a)
sugar water
b)
salt water
c)

solid sodium chloride

d)

an acidic solution like vinegar (acetic acid) or hydrochloric acid solution

54.

When the ends of two wires, from a circuit containing a battery and a lightbulb, are placed into a beaker containing an aqueous solution the light bulb glows brightly. From this observation, you can conclude the solution is probably —

a)

a weak electrolyte

b)

a strong electrolyte

c)

containing a very polar compound

d)

containing nonpolar compounds

55.

Ionic compounds undergo ___________ or split into separate ions when they dissolve in water

a)

lysis

b)

polarization

c)

decomposition

d)

disassociation

56.

Which is not a major role that electrolytes play in the human body?

a)

to send nerve signals

b)

DNA replication

c)

maintain proper pH of the blood

d)

maintain hydration

57.

Your stomach contains HCl. This gives off H+ ions when dissolved in water and gives a pH of 2. HCl is a/an

a)

acid

b)

base

c)

neutral compound

d)

nonelectrolyte

58.

What is the charge of an electron?

a)

Positive

b)

Negative

c)

Neutral

59.

Which is not a use of radioisotopes?

a)

dating formerly living things

b)

diagnosing diseases

c)

treating diseases

d)

enhancing the health of growing cells

60.

When one water molecule attracts to another, it is due to ...

a)

Ionic bonds between water molecules

b)

Covalent bonds between water molecules

c)

polar bonds between water molecules

d)

polar forces and/or hydrogen bonds between molecules

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