Term
| The total maximum number of electrons in the 3p orbitals is 6. T or F |
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Definition
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Term
| A 3p orbital is larger than a 2 p orbital. T or F |
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Definition
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Term
| The Greek symbol used in chemistry notation for 'partial" or "slightly" is δ. T or F |
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Definition
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Term
| Different wavelengths of light carry different amount of energy. T or F |
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Definition
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Term
| A polar covalent bond is more ionic than an ionic bond. T or F |
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Definition
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Term
| Electronegativities generally decrease from left to right in the Periodic Table. T or F |
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Definition
False
Electronegativities increase from left to right on the Periodic Table. |
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Term
| Water is an example of a polar molecule. T or F |
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Definition
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Term
| Phosphorous normally can be expected to form 3 bond with other elements. T or F |
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Definition
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Term
| The abbreviation for wavelength is the Greek letter ν. T or F |
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Definition
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Term
| Calcium has 4 electrons in its 4s orbital |
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Definition
False.
An s orbital only supports up to 2 electrons |
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Term
| Silicon is an example of a "d-block" element. T or F |
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Definition
False.
It's in the p-block. |
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Term
| The ionization energy for phosphorous is higher than for sodium. T or F |
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Definition
True.
P WANTS electrons. Na isn't really that interested in more electrons. |
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Term
| The octet rule must be satisfied for all the element in C2O4H2. T or F |
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Definition
False.
H follows the duet rule, not the octet rule. |
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Term
| H2O2 is an example of a diatomic molecule. T or F |
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Definition
| False.
Diatomic molecules: H2, N2, O2, F2, Cl2, Br2, and I2. |
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Term
| Triple bonds contain a total of 6 electrons. T or F |
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Definition
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Term
| The reaction between Na0 and H2O should be similar to K0 and H2O. T or F |
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Definition
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Term
| The net charge of an ionic compound must be zero. T or F |
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Definition
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Term
| Li+ has the same properties as He. T or F |
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Definition
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Term
| NH4Cl sublimed in the Separation of Mixtures laboratory. T or F |
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Definition
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Term
| The number of valence electrons = Z minus the number of core electrons. T or F |
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Definition
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Term
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. ↓
e. no arrow, there is no dipole |
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Definition
b. +→
Because N (3.0) has a higher electronegativity than Be (1.5). |
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Term
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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Definition
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Term
| N2 is:
a. a binary compound
b. an element
c. a diatomic molecule
d. a polar molecule
e. an ion |
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Definition
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Term
Metallic gold is:
a. a binary compound
b. an element
c. a diatomic molecule
d. a metalloid
e. an ion |
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Definition
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Term
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 |
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Definition
c. covalent
Be = 1.5
1.5 - 1.5 = 0.0 |
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Term
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 |
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Definition
b. polar covalent
C = 2.5 F = 4
4 - 2.5 = 1.5 |
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Term
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 |
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Definition
a. ionic
Be = 1.5
F = 4.0
4.0 - 1.5 = 2.5 |
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Term
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 |
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Definition
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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Term
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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Definition
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Term
| H2O has the molecular geometry:
a. Trigonal pyramid
b. Trigonal Planar
c. Bent or V-shaped
d. Tetrahedral
e. Ternary |
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Definition
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Term
| Is it a chemical or physical change?
Boiling liquid N2 (like I showed in class) |
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Definition
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Term
Is it a chemical or physical change?
The copper dome on St. Paul's cathedral turning blue-green |
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Definition
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Term
Is it a chemical or physical change?
Gasoline burning when you drive your car |
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Definition
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Term
Is it a chemical or physical change?
Formation of cans from molten aluminum |
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Definition
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Term
| Phosphorus electronic configuration |
|
Definition
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Term
| Phosphorus orbital box diagram |
|
Definition
[↑↓]
[↑↓] [↑↓][↑↓][↑↓]
[↑↓] [↑ ][↑ ][↑ ] |
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Term
| From the Periodic Table, what metalloid as 3d10 electrons and only 4p3 electrons? |
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Definition
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Term
| The following orbital box diagram for 1s22s22p4 is incorrect:
[↑↓] [↑↓] [↑↓][↑↓][ ]
What's the correct version? |
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Definition
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Term
| Name an example of a positively charged ion and it's elemental symbol with the correct charged ion. |
|
Definition
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Term
| Name an example of a negatively charged ion and it's elemental symbol with the correct charged ion. |
|
Definition
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Term
| Name an example of an alkaline earth metal and it's elemental symbol with the correct charged ion. |
|
Definition
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Term
| Name an example of a halogen and it's elemental symbol with the correct charged ion. |
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Definition
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Term
| Name an example of a noble gas. |
|
Definition
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Term
| Name and example of a transition metal. |
|
Definition
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Term
| Name the two types of ions. |
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Definition
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Term
| What is the isotopic symbol for Neon? |
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Definition
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Term
| How many neutrons does titanium have? |
|
Definition
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Term
| Give the correct formula for a compound containing Cr3+ and S2-: |
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Definition
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Term
| Write the correct name for MgS: |
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Definition
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Term
How many valence electrons and core electrons does each of the following have?
1. Chlorine
2. Calcium
3. Boron |
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Definition
1. Chlorine -- 7val, 10core
2. Calcium -- 2val, 18core
3. Boron-- 3val, 2core |
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Term
Give the proper name or chemical symbol for the following elements:
Nickel
Si
Potassium
Nitrogen
Carbon
S |
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Definition
Nickel -- Ni
Si -- Silicon
Potassium -- K
Nitrogen -- N
Carbon -- C
S -- Sulfur |
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Term
| Use an orbital box diagram to explain why oxygen normally can be expected to form 2 bonds in any molecule: |
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Definition
[↑↓] [↑↓] [↑↓][↑ ][↑ ]
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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Term
| What needs to surround the Lewis Dot structure for PO43-? |
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Definition
__ ___ 3-
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