Chemistry Final Exam Dr. Whitcomb Test Questions – Flashcards

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question
The total maximum number of electrons in the 3p orbitals is 6. T or F
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True
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A 3p orbital is larger than a 2 p orbital. T or F
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True
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The Greek symbol used in chemistry notation for 'partial" or "slightly" is ?. T or F
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True
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Different wavelengths of light carry different amount of energy. T or F
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True
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A polar covalent bond is more ionic than an ionic bond. T or F
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False
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Electronegativities generally decrease from left to right in the Periodic Table. T or F
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False
Electronegativities increase from left to right on the Periodic Table.
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Water is an example of a polar molecule. T or F
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True
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Phosphorous normally can be expected to form 3 bond with other elements. T or F
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True
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The abbreviation for wavelength is the Greek letter ?. T or F
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False.
? = wavelength
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Calcium has 4 electrons in its 4s orbital
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False.
An s orbital only supports up to 2 electrons
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Silicon is an example of a "d-block" element. T or F
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False.
It's in the p-block.
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The ionization energy for phosphorous is higher than for sodium. T or F
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True.
P WANTS electrons. Na isn't really that interested in more electrons.
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The octet rule must be satisfied for all the element in C2O4H2. T or F
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False.
H follows the duet rule, not the octet rule.
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H2O2 is an example of a diatomic molecule. T or F
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False.Diatomic molecules: H2, N2, O2, F2, Cl2, Br2, and I2.
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Triple bonds contain a total of 6 electrons. T or F
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True
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The reaction between Na0 and H2O should be similar to K0 and H2O. T or F
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True
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The net charge of an ionic compound must be zero. T or F
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True
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Li+ has the same properties as He. T or F
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False???
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NH4Cl sublimed in the Separation of Mixtures laboratory. T or F
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True
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The number of valence electrons = Z minus the number of core electrons. T or F
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True
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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
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b. +>
Because N (3.0) has a higher electronegativity than Be (1.5).
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KBr is:
a: a ternary compound
b: an element
c: a diatomic molecule
d: a globular cluster
e: an ionic compound
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e. an ionic compound
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N2 is:a. a binary compoundb. an elementc. a diatomic moleculed. a polar moleculee. an ion
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c. a diatomic molecule
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Metallic gold is:
a. a binary compound
b. an element
c. a diatomic molecule
d. a metalloid
e. an ion
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b. an element
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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
answer
c. covalent
Be = 1.5
1.5 - 1.5 = 0.0
question
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
answer
b. polar covalent
C = 2.5 F = 4
4 - 2.5 = 1.5
question
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
answer
a. ionic
Be = 1.5
F = 4.0
4.0 - 1.5 = 2.5
question
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
answer
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
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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
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e. 1s, 2s, 2p, 3s
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H2O has the molecular geometry:a. Trigonal pyramidb. Trigonal Planarc. Bent or V-shapedd. Tetrahedrale. Ternary
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c. Bent or V-shaped
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Is it a chemical or physical change?Boiling liquid N2 (like I showed in class)
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Physical
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Is it a chemical or physical change?

The copper dome on St. Paul's cathedral turning blue-green
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Chemical
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Is it a chemical or physical change?

Gasoline burning when you drive your car
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Chemical
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Is it a chemical or physical change?

Formation of cans from molten aluminum
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Physical
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Phosphorus electronic configuration
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1s22s22p63s23p2
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Phosphorus orbital box diagram
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[^v]
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From the Periodic Table, what metalloid as 3d10 electrons and only 4p3 electrons?
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As
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The following orbital box diagram for 1s22s22p4 is incorrect:[^v] [^v] [^v][^v][ ] What's the correct version?
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[^v] [^v] [^v][^ ][^ ]
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Name an example of a positively charged ion and it's elemental symbol with the correct charged ion.
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SodiumNa+
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Name an example of a negatively charged ion and it's elemental symbol with the correct charged ion.
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Chloride Cl-
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Name an example of an alkaline earth metal and it's elemental symbol with the correct charged ion.
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Magnesium Mg+2
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Name an example of a halogen and it's elemental symbol with the correct charged ion.
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Bromine Br-
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Name an example of a noble gas.
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Argon
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Name and example of a transition metal.
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Copper
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Name the two types of ions.
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cations and anions
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What is the isotopic symbol for Neon?
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2010Ne
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How many neutrons does titanium have?
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47.88 - 22 = 25.88 = 26
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Give the correct formula for a compound containing Cr3+ and S2-:
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Cr2S3:
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Write the correct name for MgS:
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magnesium sulfide
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How many valence electrons and core electrons does each of the following have?
1. Chlorine
2. Calcium
3. Boron
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1. Chlorine -- 7val, 10core
2. Calcium -- 2val, 18core
3. Boron-- 3val, 2core
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Give the proper name or chemical symbol for the following elements:
Nickel
Si
Potassium
Nitrogen
Carbon
S
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Nickel -- Ni
Si -- Silicon
Potassium -- K
Nitrogen -- N
Carbon -- C
S -- Sulfur
question
Use an orbital box diagram to explain why oxygen normally can be expected to form 2 bonds in any molecule:
answer
[^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.
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What needs to surround the Lewis Dot structure for PO43-?
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__ ___ 3-
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