CHM 1032-0001

Exam 1 Fall 2020

Instructor: Name:Date:

1. What are the basic SI units of length?

a. mile

b. inch

c. meter

d. centimeter

e. All of the above

2. Group 2A elements are called?

a. Alkali Earth Metals

b. Alkaline Earth Metals

c. Both A and B

d. None of the above

3. The exponential 104 is equal to which decimal number?

a. 10

b. 10,000

c. 1

d. 1,000

e. None of the above

4. The correct number of significant figures in the number 1.2501 • 10-3 is:

a. 5

b. 7

c. 4

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d. ambiguous

e. none of the above

5. How many significant figures should be reported in the answer to the following calculation?

(95.43)(63.002)(0.0090)a. 3

b. 4

c. 2

d. 1

e. None of the above

6. How many cm3 are in 2.5m3

a. 2.5 x 106

b. 2.5 x 10-2

c. 2.5 x 102

d. 2.5 x 10-6

e. None of the above

7. The jet fuel in an airplane has a mass of 97.5kg and a density of 0.804g/cm3. What is the volume of this jet fuel?

a. 1.21 x 105 cm3

b. 7.84 x 10-2 cm3

c. 7.84 x 104 cm3

d. 1.21 x 102 cm3

8. How many significant figures should be reported in the answer to the following calculation?

(43.980) x (19.0023+25)=

a. 3

b. 2

c. 4

d. 1

e. None of the above

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9. A radiolabeled isotope of sodium-24 contains:

a. 11 protons, 11 neutrons, 11 electrons

b. 24 protons, 11 neutrons, 24 electrons

c. 11 protons, 13 neutrons, 11 electrons

d. 11 protons, 13 neutrons, 11 electrons

e. None of the above

10. What is the density of a block that is 12.0cm x 6.00cm x 2.00 cm and has a mass of 356g

a. 1.00g/cm3

b. 4.95 g/cm3

c. 3.56 g/cm3

d. 2.47 g/cm3

e. None of the above

11. A chemist mixes sodium with water and witnesses a violent reaction between the metal and water. This is best classified as

a. An observation

b. A hypothesis

c. A law

d. A theory

12. All of the following statements in Dalton’s atomic theory are true EXCEPT

a. Each element is composed of tiny indestructible particles called atoms

b. Atoms combine in simple, whole number ratios to form compounds

c. Atoms of one element can change into atoms of another element

d. All atoms of a given element cannot change into atoms of another element

13. How many valence electrons are drawn for a phosphorus atom using Lewis structure?

a. 5

b. 4

c. 3

d. 2

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e. none of the above

14. Which element has the smallest atomic radius?

a. C

b. Si

c. Be

d. F

e. none of the above

15. When potassium forms an ion, it loses electrons, how many electrons does it lose, and in which orbital(s) do the electrons come from

a. 1 electron; one from the 3s orbital

b. 5 electrons; two from the 3s orbital and three from the 3p orbital

c. 2 electrons; one from the 4s orbital and one from the 4p orbital

d. 1 electron; one from the 4s orbital

e. none of the above

16. What is the electron configuration for Ge?

a. 1s22s22p63s23p64s24d104p2

b. 1s22s23p64s25s26d107p2

c. 1s22s22p63s23p64s23d104p2

d. 1s22s22p63s23p63d104s24p2

e. none of the above

17. Which electron transition in the Bohr model would produce electromagnetic radiation with the highest energy?

a. n=2n=1

b. n=3n=2

c. n=5n=4

d. n=4n=3

e. none of the above

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18. What is the correct order of the electromagnetic spectrum from lowest frequency to highest frequency?

a. Gamma RaysX-RaysVisible LightUltraviolet RadiationInfrared RadiationMicrowavesRadio Waves

b. Gamma RaysX-RaysInfrared RadiationUltraviolet RadiationVisible Light MicrowavesRadio Waves

c. Radio WavesMicrowavesUltraviolet RadiationVisible Light Infrared RadiationX-RaysGamma Rays

d. Radio WavesMicrowavesInfrared RadiationVisible Light Ultraviolet RadiationX-RaysGamma Rays

e. Gamma RaysRadio WavesX-RaysInfrared RadiationUltraviolet RadiationVisible Light

19. How many unpaired orbitals are in chlorine?

a. 4

b. 3

c. 2

d. 1

e. None of the above

20. An atoms valence electrons are those important in?

a. physical bonding

b. intermolecular forces

c. intramolecular forces

d. chemical bonding

e. none of the above

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Disclaimer: I have made this review to the best of my ability. It is not comprehensive and should only be used as an aid to your review, not as your only study tool. All the problems are from Tro, Nivaldo J. Chemistry a Molecular Approach 4th ed., Pearson/Prentice Hall, 2017 and in collaboration with problems from Dr. Amel Garbou

Zero Rules

1. All nonzero digits are significant.1.05 0.0110

2. Interior zeros (zeros between two numbers) are significant.I.208 50.1

3. Trailing zeros (zeros to the right of a nonzero number) that fall after a decimal point are significant. 5.10 3.00

4. Trailing zeros that fall before a decimal point are significant. 50.00 1700.24

5. Leading zeros (zeros to the left of the first nonzero number) are NOT significant. They only serve to locate the decimal point.

0.00056. Trailing zeros at the end of a number, but before an implied decimal point, are

ambiguous and should be avoided.

350 350.0 3.5 x 102

(two significant figures) Or 3.50 x 102

(three significant figures)

Multiplication and Division Rule

The result of multiplication or division carries the same number of significant figures as the factor with the fewest significant figures.

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Addition and Subtraction

In addition or subtraction calculations, the result carries the same number of decimal places as the quantity carrying the fewest decimal places

Combined Operations

When doing calculations that involve both multiplication or division and addition or subtraction, first do a calculation for the operation shown in parenthesis and round that value to the correct number of significant figures, then use the rounded number to carry out the next operation.

EM spectrum

28. Orbitals fill in the following order: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s

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29. Valence electrons are the electrons in the outermost shell (look for highest number in front of the letters and that’s your outermost shell

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Main Group elements information

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