Chapter 1
Differentiate between electrons, protons, and neutrons
Electrons: *Negative charge, orbits nucleus, 0 amu*
Protons: *Positive charge, located in nucleus, 1 amu*
Neutrons: *No charge, located in nucleus, 1 amu*
What are the four rules when determining the number of significant figures in a numerical value?
1. Non-zero digits are always significant
2. Any zeros between two significant digits are significant
3. Trailing zeros (those at the end) are significant only if the number contains a decimal point
4. Zeros to left of the first nonzero digit are insignificant
Determine the value for l when an electron is in subshell:
s:
p:
d:
f:
s: 0
p: 1
d: 2
f: 3
Determine where each of the trends increases:
Ionization Energies
Electron Affinity
Atomic Size of Neutral Atoms
Ionization Energies: Increase right and up
Electron Affinity: Increases right and up
Atomic Size of Neutral Atoms: Increases left and down
Give the name or formula for:
1. Magnesium Chloride
2. CCl4
3. NO
1. MgCl2
2. Carbon Tetrachloride
3. Nitrogen Monoxide
Classify each type of matter as element, compound, heterogeneous mixture, or homogeneous mixture
1. Kool-aid
2. O2
3. Air
4. Sand
5. Ammonia
1. Homogeneous mixture
2. Element
3. Homogeneous mixture
4. Heterogeneous mixture
5. Compound
1. What is the significant figure rule regarding addition and subtraction problems?
2. What is the significant figure rule regarding multiplication and division problems?
1. Final answers are limited to the place holder of the measurement with the largest place holder for its final sig fig
2. Final answers are limited to the same number of significant figures as the measurement with the fewest significant figures
How many orbitals are in subshell?
s:
p:
d:
f:
s: 1
p: 3
d: 5
f: 7
Determine the electron configuration for:
1. Beryllium
2. Sodium
3. Sulfur
1. 1s2 2s2
2. 1s2 2s2 2p6 3s1
3. 1s2 2s2 2p6 3s2 3p4
Give the name or formula for:
1. SnCl4
2. Silver (I) Sulfide
3. P4O10
4. ICl
1. Tin (IV) Chloride
2. Ag2S
3. Tetraphosphorus Decaoxide
4. Iodine Monochloride
Name the four parts to Dalton's Atomic Theory.
1. Each element is composed of tiny, indestructible particles called atoms.
2. All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements.
3. Atoms combine in simple, whole-number ratios to form compounds
4. Atoms of one element cannot change into atoms of another element.
What is the difference between precision and accuracy?
Precision: Refers to how close a series of measurements are to one another
Accuracy: Refers to how close a measured value is to the actual value
Determine the n and l values for:
3p
4f
2s
3p: n=3, l=1
5f: n=5, l=3
2s: n=2, l=0
Determine the electron configuration for:
1. I-
2. Zn+2
3. Gallium
1. [Xe]
2. [Ar] 3d10
3. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1
Name or give the formula for the following polyatomic ions:
1. Nitrite
2. SO4-2
3. ClO-
1. NO2-
2. Sulfate
3. Hypochlorite
Create the ion notation for each below:
1. P- 20, N- 24, E- 20
2. P- 8, N- 9, E- 8
3. P- 39, N- 50, E- 39
4. P- 11, N- 12, E- 11
1. 44Ca
2. 17O
3. 89Y
4. 23Na
Determine the number of sig figs for each problem below:
1. 153 mL + 1.8 mL + 9.16 mL
2. 0.954 - 0.3109
3. 12.5849 + 2.4
1. 164 mL
2. 0.643 units
3. 15.0 units
Answer the following questions:
1. The longer the wavelength, the ? the frequency.
2. Which has more energy: ultraviolet or infrared light?
3. Rank these colors from smallest to largest energy: Blue, yellow, orange
1. Shorter
2. Ultraviolet
3. Orange, yellow, blue
Determine which is more metallic in each pair:
1. Sodium or Potassium
2. Oxygen or Chlorine
3. Zinc or Copper
1. Potassium
2. Oxygen
3. Copper
Give the formula mass for:
1. CuSO4
2. CaCOH
3. K3PO4
1. 159.5 g/mol
2. 69.09 g/mol
3. 212.3 g/mol
Create the isotope notation for each below:
1. P- 9, N- 11, E- 10
2. P- 26, N- 30, E- 24
3. P- 1, N- 0, E- 2
4. P- 24, N- 28, E- 21
1. 20F1-
2. 56Fe2+
3. 1H1-
4. 52Cr3+
Determine the number of sig figs for each problem below:
1. (2.5 m) x (2.01 m) x (2.755 m)
2. 16.15 / 2.7
3. (0.003 / 5)
1. 14 m3
2. 6.0 units
3. 0.0006 units
Write a set of quantum numbers for:
1. 4p orbital
2. 2s orbital
3. 4d orbital
1. n=4, l=1, ml= -1 to +1
2. n=2, l=0, ml=0
3. n=4, l=2, ml= -2 to +2
Organize the groups from largest to smallest atomic radius
1. Kr, Xe, Ne, O
2. H, He, Se, Ca
1. Xe > Kr > O > Ne
2. Ca > Se > He > H