Unit 2 Review

actorrattleUrban and Civil

Nov 15, 2013 (3 years and 4 months ago)

62 views

Unit 2 Review


Modified True/False

Indicate whether the sentence or statement is true or false. If false, change the identified word or phrase to make the
sentence or statement true.


____

1.

Bohr's atomic theory states that electrons may only possess spe
cific amounts of
energy
.
____________________


____

2.

The quantum mechanical model of the atom is capable of determining the
exact

location of an electron in an
atom. ____________________


____

3.

All alkali earth metals have valence electrons in
s orbita
ls

when they are in their ground state.
____________________


____

4.

The hydrogen atom will produce a
complete

spectrum when it is energized. ____________________


____

5.

Schrodinger's equation describes the electron as a
wave
. ____________________


____

6.

Transition metals are
monovalent

because they attempt to get more stable electron configurations like half
-
filled and empty orbitals. ____________________


____

7.

The 2p orbitals in oxygen have
three

unpaired electrons. ____________________


____

8.

T
he shape of SO
2

is
trigonal planar
. ____________________


____

9.

Absorption spectra are the result of energy that has been
absorbed
by electrons. ____________________


____

10.

Electrons are most likely found near the
nucleus
, regardless of the type of or
bital they 'occupy'.
____________________


____

11.

The Pauli exclusion principle requires that two electrons in the same orbital have
the same spin
.
____________________


____

12.

Quantum mechanics involves using probabilities to determine the shape of
an

atom
. ____________________


____

13.

The electron configuration for
sulfur, S
is shown below. _________________________

































____

14.

The valence p orbitals in phosphorus, P, are
half
-
filled
. _________________
___


____

15.

All of the valence electrons in Fe
2+

must

have the same spin. _________________________


____

16.

Hund's rule

states that you must fill electrons into the lowest energy levels first.
_________________________


____

17.

A laser produces
monoch
romatic
light. _________________________


____

18.

Spectrophotometers
cannot

be used for qualitative observations. _________________________


____

19.

X
-
rays are made up of extremely high energy
photons.
_________________________


____

20.

MRI stands for
m
agnetic reflection imaging
. ______________________________


____

21.

A photon of light is equal to one
quantum

of energy. ____________________


____

22.

Superconductors are substances that conduct electricity with extremely low
voltage
.
___________________
______


____

23.

The energy of electrons is quantized as
photons
. _________________________


____

24.

Ionic compounds have
higher

melting points than molecular compounds because of strong attractive forces
between particles. _________________________


____

25.

The shape of boron trifluoride, BF
3
, is
tetrahedral
. ______________________________


____

26.

VSEPR theory predicts molecular shapes based on keeping
protons

as far apart as possible.
_________________________


____

27.

Carbon tetrafluoride, CF
4
, cont
ains four polar bonds and is a
polar

molecule. _________________________


____

28.

The surface tension of water is due to the
hydrogen bonding

between water molecules.
_________________________


____

29.

A molecule whose central atom is surrounded by two l
one pairs and four atoms will have a
square planar

shape. _________________________


____

30.

CH
3
Cl is a
polar

molecule. _________________________


____

31.

An ionic compound would be expected to have a
low

melting point. _________________________


____

32
.

Diamond does not conduct electricity because it contains
delocalized electrons
.
______________________________


____

33.

Molten or dissolved ionic compounds conduct electricity because they contain
delocalized electrons
.
_________________________


____

3
4.

Sulfur dioxide, SO
2
, is a bent molecule with a bond angle that is slightly less than
109
o
.
_________________________


____

35.

Xenon tetrafluoride, XeF
4
, is a
tetrahedral
molecule. _________________________


____

36.

Methane, CH
4
, contains
polar

bonds.
_________________________


____

37.

Carbon dioxide, CO
2
, is a
polar

molecule. _________________________


____

38.

Water is adhesive because it is
bi
-
polar
. _________________________


____

39.

Hydrogen bonding

may explain why ice is less dense than liquid w
ater. _________________________


____

40.

Dr. Richard Bader uses computers to create electron density maps for
large complex molecules.
______________________________


____

41.

Dr. Robert LeRoy developed a technique for determining
bond lengths
. __________
____________________


____

42.

Dr. Robert LeRoy is interested in
intermolecular

forces. _________________________


____

43.

A dipole occurs when two atoms with
similar

electronegativities bond to each other.
_________________________


Completion

Complete e
ach sentence or statement.



44.

A region in which there is a high probability of finding an electron is called an ____________________.



45.

Bohr's model works perfectly for ____________________.



46.

____________________ determined that it is impossibl
e to predict the exact location of an electron.



47.

____________________ orbitals are non
-
directional.



48.

There are ____________________ different orientations in space for p
-
orbitals.



49.

When an electron is in its lowest energy level, it is in the

____________________.



50.

In his model of the atom, Bohr identified each energy level using an integer,
n
, and called it the
___________________________________.



51.

Cl
1
-
, Ar and Ca
2+

are ____________________.



52.

____________________ are high energ
y electromagnetic radiation.



53.

____________________ produce parallel, monochromatic light.



54.

Spin changes in hydrogen nuclei of water molecules can be detected using
______________________________.



55.

At extremely low temperatures, helium is a _
___________________.



56.

S
-
block elements are all ____________________.



57.

A photon is a ____________________ of light.



58.

The electron configuration for ____________________ is 1s
2
2s
2
2p
6
3s
2
3p
6
.



59.

The oxide, O
2
-
, is ____________________ with ne
on, Ne.



60.

The "1" in helium's (He) electron configuration represents the ____________________.



61.

The concept of the duality of matter means that an electron is both a particle and a _____________________.



62.

The surface tension of water is due t
o the _________________________ between its particles.



63.

____________________ of electrons take up more room than bonded pairs.



64.

The shape of sulfur dioxide would most likely be ____________________.



65.

The shape of MnI
5

would most likely be __
____________________________.



66.

The metal ions in a metallic solid are surrounded by delocalized electrons because metals have low
_________________________.



67.

The shape of sulphur hexachloride, SCl
6
, is ____________________.



68.

The shape of met
hane, CH
4
, is ____________________.



69.

The shape of ammonia, NH
3
, is ______________________________.



70.

The shape of xenon tetrafluoride, XeF
4
, is _________________________.



71.

The shape of beryllium fluoride, BeF
2
, is ____________________.



72.

The shape of boron trihydride, BH
3
, is _________________________.



73.

The shape of hydrogen sulfide, H
2
S, is ____________________.



74.

The shape of phosphorus pentahydride, PH
5
, is ___________________________________.



75.

VSEPR theory predicts the __
__________________ of molecules.



76.

The molecules in any glue must have the ability to ____________________ with molecules of other
substances.



77.

_________________________ tend to be brittle.



78.

Due to its structure, diamond is classified as a __
_______________________.



79.

The electrostatic forces between ions in ionic compounds cause ____________________ boiling points.



80.

Insects can walk on water because of ______________________________.



81.

Dispersion forces are ____________________ t
han covalent bonds.



82.

Adhesive properties of glues can be explained by examining _________________________ forces.



83.

The large difference in electronegativities between hydrogen and chlorine produces a
____________________ in the hydrogen chloride
molecule.


Essay



84.

Ernest Rutherford is known as the father of nuclear chemistry. Describe his Gold Foil experiment and then
explain how he used this experimental evidence to hypothesize about the existence of a nucleus.



85.

Compare and contrast the
Bohr
-
Rutherford model of the atom with the quantum mechanical model.



86.

Explain, in your own words, how Bohr developed his model of the atom.



87.

Explain water's properties using what you know about its inter
-

and intramolecular forces.



88.

Explain
VSEPR theory in your own words. Use examples.



89.

We are able to "see" the shapes of molecules with X
-
ray crystallography. However, even without this
technology, there is a great deal of evidence that water, H
2
O, is a bent, polar molecule. Discuss this e
vidence
and explain how it relates to our model of the water molecule.



90.

Explain, in your own words, how to determine the polarity of a substance. Use examples if you wish.



91.

Describe, in your own words, two allotropes of carbon. Include a comparis
on of physical and chemical
properties.



92.

Describe some contributions that Canadians have made to the scientific community's understanding of the
structures and properties of chemicals.

Unit 2 Review

Answer Section


MODIFIED TRUE/FALSE



1.

ANS:

T



R
EF:

K/U

OBJ:

3.4

LOC:

SP1.01



2.

ANS:

F, probable



REF:

K/U

OBJ:

3.7

LOC:

SP1.02



3.

ANS:

T



REF:

K/U

OBJ:

3.6

LOC:

SP1.03



4.

ANS:

F, line



REF:

K/U

OBJ:

3.4

LOC:

SP1.01



5.

ANS:

T



REF:

K/U

OBJ:

3.7

LOC:

SP1.02



6.

ANS:

F, multi
-
valent



REF:

K/
U

OBJ:

3.6

LOC:

SP1.03



7.

ANS:

F, two



REF:

I

OBJ:

3.5

LOC:

SP1.02



8.

ANS:

F

bent

angular


REF:

I

OBJ:

4.3

LOC:

SP2.03



9.

ANS:

T



REF:

K/U

OBJ:

3.4

LOC:

SP1.01



10.

ANS:

T



REF:

K/U

OBJ:

3.5

LOC:

SP1.02



11.

ANS:

F, different spins


REF:

K/U

OBJ
:

3.6

LOC:

SP2.01



12.

ANS:

F

an orbital

orbitals


REF:

K/U

OBJ:

3.7

LOC:

SP2.01



13.

ANS:

F, chlorine, Cl



REF:

I

OBJ:

3.6

LOC:

SP2.02



14.

ANS:

T



REF:

I

OBJ:

3.6

LOC:

SP2.02



15.

ANS:

F

can

might


REF:

I

OBJ:

3.6

LOC:

SP2.02



16.

ANS:

F, Auf bau
principle


REF:

K/U

OBJ:

3.6

LOC:

SP2.02



17.

ANS:

T



REF:

MC

OBJ:

3.8

LOC:

SP3.01



18.

ANS:

F, can



REF:

MC

OBJ:

3.8

LOC:

SP3.01



19.

ANS:

T



REF:

MC

OBJ:

3.8

LOC:

SP3.01



20.

ANS:

F, magnetic resonance imaging

REF:

MC

OBJ:

3.8

LOC:

SP3.01



21.

AN
S:

T



REF:

K/U

OBJ:

3.3

LOC:

SP1.01



22.

ANS:

F, resistance



REF:

MC

OBJ:

3.7

LOC:

SP3.02



23.

ANS:

T



REF:

K/U

OBJ:

3.3

LOC:

SP1.01



24.

ANS:

T



REF:

K/U

OBJ:

4.6

LOC:

SP2.05



25.

ANS:

F, trigonal planar


REF:

I

OBJ:

4.3

LOC:

SP2.03



26.

ANS:

F,
electron pairs


REF:

K/U

OBJ:

4.3

LOC:

SP1.05



27.

ANS:

F, non polar



REF:

I

OBJ:

4.4

LOC:

SP2.04



28.

ANS:

T



REF:

K/U

OBJ:

4.5

LOC:

SP1.04



29.

ANS:

T



REF:

K/U

OBJ:

4.3

LOC:

SP1.03



30.

ANS:

T



REF:

I

OBJ:

4.4

LOC:

SP2.04



31.

ANS:

F, high



RE
F:

I

OBJ:

4.6

LOC:

SP2.05



32.

ANS:

F, no delocalized electrons

REF:

K/U

OBJ:

4.6

LOC:

SP1.04



33.

ANS:

F, [mobile] ions


REF:

K/U

OBJ:

4.6

LOC:

SP1.04



34.

ANS:

F, 120
o



REF:

I

OBJ:

4.3

LOC:

SP2.03



35.

ANS:

F, square planar


REF:

I

OBJ:

4.3

LOC:

SP2
.03



36.

ANS:

T



REF:

I

OBJ:

4.4

LOC:

SP2.04



37.

ANS:

F, non polar



REF:

I

OBJ:

4.4

LOC:

SP2.04



38.

ANS:

F, polar



REF:

K/U

OBJ:

4.5

LOC:

SP1.04



39.

ANS:

T



REF:

K/U

OBJ:

4.5

LOC:

SP1.04



40.

ANS:

F, small simple molecules

REF:

MC

OBJ:

4.3

LOC:

SP3.03



41.

ANS:

F, small molecule radii

REF:

MC

OBJ:

4.5

LOC:

SP3.03



42.

ANS:

T



REF:

MC

OBJ:

4.5

LOC:

SP3.03



43.

ANS:

F, very different


REF:

I

OBJ:

4.4

LOC:

SP2.01


COMPLETION



44.

ANS:

orbital



REF:

C

OBJ:

3.5

LOC:

SP2.01



45.

ANS:

hydrogen



REF:

K/U

OBJ:

3.4

LOC:

SP1.01



46.

ANS:

Heisenberg



REF:

K/U

OBJ:

3.7

LOC:

SP1.02



47.

ANS:

S



REF:

K/U

OBJ:

3.6

LOC:

SP1.03



48.

ANS:

three



REF:

K/U

OBJ:

3.6

LOC:

SP1.03



49.

ANS:

ground state



REF:

K/U

OBJ:

3.4

LOC:

SP1.01



50.

ANS:

principal
quantum number

REF:

K/U

OBJ:

3.4

LOC:

SP1.01



51.

ANS:

iso
-
electronic



REF:

K/U

OBJ:

3.6

LOC:

SP1.03



52.

ANS:

X
-
rays



REF:

MC

OBJ:

3.8

LOC:

SP3.01



53.

ANS:

Lasers



REF:

MC

OBJ:

3.8

LOC:

SP3.01



54.

ANS:


MRI

magnetic resonance imaging


REF:

MC

OBJ
:

3.8

LOC:

SP3.01



55.

ANS:

superconductor


REF:

MC

OBJ:

3.7

LOC:

SP3.02



56.

ANS:

metals



REF:

K/U

OBJ:

3.6

LOC:

SP1.03



57.

ANS:


packet

particle


REF:

C

OBJ:

3.3

LOC:

SP2.01



58.

ANS:

argon



REF:

C

OBJ:

3.6

LOC:

SP2.02



59.

ANS:

iso
-
electronic



REF:

C

OBJ:

3.6

LOC:

SP2.02



60.

ANS:

energy level



REF:

C

OBJ:

3.6

LOC:

SP2.02



61.

ANS:

wave



REF:

K/U

OBJ:

3.7

LOC:

SP1.02



62.

ANS:

hydrogen bonding


REF:

K/U

OBJ:

4.5

LOC:

SP1.04



63.

ANS:


Unbonded pairs

Lone pairs


REF:

K/U

OBJ:

4.3

LOC:

SP1.0
5



64.

ANS:

bent



REF:

I

OBJ:

4.3

LOC:

SP2.03



65.

ANS:

square pyramidal


REF:

I

OBJ:

4.3

LOC:

SP2.03



66.

ANS:

electron affinity


REF:

K/U

OBJ:

4.6

LOC:

SP1.04



67.

ANS:

octahedral



REF:

I

OBJ:

4.3

LOC:

SP2.03



68.

ANS:


tetrahedral

tetrahedron


RE
F:

I

OBJ:

4.3

LOC:

SP2.03



69.

ANS:


trigonal pyramidal

trigonal pyramid


REF:

I

OBJ:

4.3

LOC:

SP2.03



70.

ANS:

square planar



REF:

I

OBJ:

4.3

LOC:

SP2.03



71.

ANS:

linear



REF:

I

OBJ:

4.3

LOC:

SP2.03



72.

ANS:

trigonal planar



REF:

I

OBJ:

4.3

LOC:

SP2.03



73.

ANS:

bent



REF:

I

OBJ:

4.3

LOC:

SP2.03



74.

ANS:

trigonal bipyramidal


REF:

I

OBJ:

4.3

LOC:

SP2.03



75.

ANS:

shape



REF:

K/U

OBJ:

4.3

LOC:

SP1.05



76.

ANS:

bond



REF:

MC

OBJ:

4.5

LOC:

SP1.04



77.

ANS:


Ionic compounds

Salts


REF:

I

OBJ:

4.6

LOC:

SP2.05



78.

ANS:

network solid



REF:

I

OBJ:

4.6

LOC:

SP2.05



79.

ANS:

high



REF:

I

OBJ:

4.6

LOC:

SP2.05



80.

ANS:

hydrogen bonding


REF:

K/U

OBJ:

4.5

LOC:

SP1.04



81.

ANS:

weaker



REF:

K/U

OBJ:

4.6

LOC:

SP1.04



82.

ANS:

intermolecular



R
EF:

MC

OBJ:

4.5

LOC:

SP3.02



83.

ANS:

dipole



REF:

C

OBJ:

4.4

LOC:

SP2.04