Chemistry Final Exam Dr. Whitcomb

The total maximum number of electrons in the 3p orbitals is 6. T or F
True
A 3p orbital is larger than a 2 p orbital. T or F
True
The Greek symbol used in chemistry notation for ‘partial” or “slightly” is ?. T or F
True
Different wavelengths of light carry different amount of energy. T or F
True
A polar covalent bond is more ionic than an ionic bond. T or F
False
Electronegativities generally decrease from left to right in the Periodic Table. T or F
False
Electronegativities increase from left to right on the Periodic Table.
Water is an example of a polar molecule. T or F
True
Phosphorous normally can be expected to form 3 bond with other elements. T or F
True
The abbreviation for wavelength is the Greek letter ?. T or F
False.
? = wavelength
Calcium has 4 electrons in its 4s orbital
False.
An s orbital only supports up to 2 electrons
Silicon is an example of a “d-block” element. T or F
False.
It’s in the p-block.
The ionization energy for phosphorous is higher than for sodium. T or F
True.
P WANTS electrons. Na isn’t really that interested in more electrons.
The octet rule must be satisfied for all the element in C2O4H2. T or F
False.
H follows the duet rule, not the octet rule.
H2O2 is an example of a diatomic molecule. T or F
False.Diatomic molecules: H2, N2, O2, F2, Cl2, Br2, and I2.
Triple bonds contain a total of 6 electrons. T or F
True
The reaction between Na0 and H2O should be similar to K0 and H2O. T or F
True
The net charge of an ionic compound must be zero. T or F
True
Li+ has the same properties as He. T or F
False???
NH4Cl sublimed in the Separation of Mixtures laboratory. T or F
True
The number of valence electrons = Z minus the number of core electrons. T or F
True
Electronegativities: H = 2.1, Be = 1.5, N = 3.0, F = 4.0, O = 3.5

The correct dipole moment arrow for a Be-N bond is:

a. <+
b. +>
c. ^
d. v
e. no arrow, there is no dipole

b. +>
Because N (3.0) has a higher electronegativity than Be (1.5).
KBr is:
a: a ternary compound
b: an element
c: a diatomic molecule
d: a globular cluster
e: an ionic compound
e. an ionic compound
N2 is:a. a binary compoundb. an elementc. a diatomic moleculed. a polar moleculee. an ion
c. a diatomic molecule
Metallic gold is:
a. a binary compound
b. an element
c. a diatomic molecule
d. a metalloid
e. an ion
b. an element
Electronegativities: H = 2.1, Be = 1.5, N = 3.0, F = 4.0, O = 3.5

The type of bond in Be-Be is:
a. ionic
b. polar covalent
c. covalent
d. polar ionic
e. unstable

c. covalent
Be = 1.5
1.5 – 1.5 = 0.0
Electronegativities: H = 2.1, Be = 1.5, N = 3.0, F = 4.0, O = 3.5

The type of bond in C-F is:
a. ionic
b. polar covalent
c. covalent
d. polar ionic
e. unstable

b. polar covalent
C = 2.5 F = 4
4 – 2.5 = 1.5
Electronegativities: H = 2.1, Be = 1.5, N = 3.0, F = 4.0, O = 3.5

The type of bond in Be-F is:
a. ionic
b. polar covalent
c. covalent
d. polar ionic
e. unstable

a. ionic
Be = 1.5
F = 4.0
4.0 – 1.5 = 2.5
Electronegativities: H = 2.1, Be = 1.5, N = 3.0, F = 4.0, O = 3.5

The correct order of the following bonds from least polar to most polar is:
a. Be-C, Be-N, H-F, O-O
b. H-F, O-O, Be-N, Be-C
c. Be-N, Be-C, O-O, H-F
d. O-O, Be-C, Be-N, H-F
e. O-O, Be-N, H-F, Be-C

d. O-O, Be-C, Be-N, H-F
O-O 3.5 – 3.5 = 0.0 Least Polar
Be-C 1.5-2.5 = 1.0
Be-N 1.5-3.0 = 1.5
H-F 4.0-2.1 = 1.9 Most Polar
The order of orbital filling begins with:

a. 1s, 2s, 2d, 2p
b. 3s, 2p, 2s, 1s
c. 1s, 2s, 2p, 2d
d. 1s, 2s, 3s, 4s
e. 1s, 2s, 2p, 3s

e. 1s, 2s, 2p, 3s
H2O has the molecular geometry:a. Trigonal pyramidb. Trigonal Planarc. Bent or V-shapedd. Tetrahedrale. Ternary
c. Bent or V-shaped
Is it a chemical or physical change?Boiling liquid N2 (like I showed in class)
Physical
Is it a chemical or physical change?

The copper dome on St. Paul’s cathedral turning blue-green

Chemical
Is it a chemical or physical change?

Gasoline burning when you drive your car

Chemical
Is it a chemical or physical change?

Formation of cans from molten aluminum

Physical
Phosphorus electronic configuration
1s22s22p63s23p2
Phosphorus orbital box diagram
[^v]
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From the Periodic Table, what metalloid as 3d10 electrons and only 4p3 electrons?
As
The following orbital box diagram for 1s22s22p4 is incorrect:[^v] [^v] [^v][^v][ ] What’s the correct version?
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Name an example of a positively charged ion and it’s elemental symbol with the correct charged ion.
SodiumNa+
Name an example of a negatively charged ion and it’s elemental symbol with the correct charged ion.
Chloride Cl
Name an example of an alkaline earth metal and it’s elemental symbol with the correct charged ion.
Magnesium Mg+2
Name an example of a halogen and it’s elemental symbol with the correct charged ion.
Bromine Br
Name an example of a noble gas.
Argon
Name and example of a transition metal.
Copper
Name the two types of ions.
cations and anions
What is the isotopic symbol for Neon?
2010Ne
How many neutrons does titanium have?
47.88 – 22 = 25.88 = 26
Give the correct formula for a compound containing Cr3+ and S2-:
Cr2S3:
Write the correct name for MgS:
magnesium sulfide
How many valence electrons and core electrons does each of the following have?
1. Chlorine
2. Calcium
3. Boron
1. Chlorine — 7val, 10core
2. Calcium — 2val, 18core
3. Boron– 3val, 2core
Give the proper name or chemical symbol for the following elements:
Nickel
Si
Potassium
Nitrogen
Carbon
S
Nickel — Ni
Si — Silicon
Potassium — K
Nitrogen — N
Carbon — C
S — Sulfur
Use an orbital box diagram to explain why oxygen normally can be expected to form 2 bonds in any molecule:
[^v] [^v] [^v][^ ][^ ]
1s2 2s2 2p4

Oxygen can be expected to form 2 bonds in any molecule because, as illustrated by the orbital box diagram, there are 2 “vacancies” in the 2 p orbital which O would like to fill with 2e-, thereby resulting in an electron configuration like that of a noble gas.

What needs to surround the Lewis Dot structure for PO43-?
__ ___ 3-
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