Final Exam 1-4

Question 1

Question

The statement, Matter is neither creater nor destoryed is called

Answer

Law of Conservation of Mass
Law of Definite Proportions
Dalton's Atomic Theory
The Scientific Method
Law of Multiple Proportions

Question 2

Question

All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to?

Answer

Law of Definite Proportions
Law of the Conservation of Mass
Law of Modern Atomic Theory
Law of Multiple Proportions
First Law of Thermodynamics

Question 3

Question

Which of the following is an example of the law of multiple proportions?

Answer

A sample of chlorine is found to contain three times as much Cl-35 as Cl-37
Two different compounds formed from carbon and oxygen have the following mass ratios: 1.33 g O :1 g C and 2.66 g O :1 g C
Two different samples of table salt are found to have the same ratio of sodium to chloride
The atomic mass of bromine is found to be 79.9 amu
Nitrogen dioxide always has a mass ratio of 2.28g O : 1 g N

Question 4

Question

Calculate the atomic mass of element "X," if it has 2 naturally occurring isotopes with the following masses and natural abundances. X-45 44.8776 amu 32.88% X-47 46.9443 amu 67.12%

Answer

46.26 amu
45.91 amu
46.34 amu
46.84 amu
44.99 amu

Question 5

Question

122 Given the element X 82 How many electrons does this element have? [blank_start]82[blank_end] How many protons? [blank_start]82[blank_end] How many neutrons? [blank_start]40[blank_end] What is the element? [blank_start]Pb[blank_end]

Answer

Question 6

Question

How many iron atoms are contained in 354 g of iron?

Answer

2.62 × 1025 Fe atoms
2.13 × 1026 Fe atoms
4.69 × 1024 Fe atoms
3.82 × 1024 Fe atoms
9.50 × 1022 Fe atoms

Question 7

Question

Determine the density of an object that has a mass of 149.8 g and displaces 12.1 mL of water when placed in a graduated cylinder.

Answer

8.08 g/mL
1.38 g/mL
12.4 g/mL
18.1 g/mL
11.4 g/mL

Question 8

Question

What answer should be reported, with the correct number of significant figures, for the following calculation? (433.621 - 333.9) × 11.900

Answer

1.19 × 103
1.187 × 103
1.1868 × 103
1.18680 × 103
1.186799 × 103

Question 9

Question

How many significant figures are in the measurement, 0.00049320 g?

Answer

Question 10

Question

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

Answer

229 nm
436 nm
206 nm
485 nm
675 nm

Question 11

Question

Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89 × 1014 Hz.

Answer

3.09 × 10-19 J
6.14 × 10-19 J
3.24 × 10-19 J
1.63 × 10-19 J
5.11 × 10-19 J

Question 12

Question

How many orbitals are contained in n=1 ([blank_start]1s[blank_end]), in n=2 ([blank_start]1s+3p[blank_end]), in n=3 ([blank_start]1s+3p+5d[blank_end]), in n=6 ([blank_start]1s+3p+5d+7f[blank_end])

Answer

1s
1s+3p
1s+3p+5d
1s+3p+5d+7f

Question 13

Question

Determine the energy change associated with the transition from n=2 to n=5 in the hydrogen atom.

Answer

-2.18 × 10-19 J
+6.54 × 10-19 J
+4.58 × 10-19 J
-1.53 × 10-19 J
+3.76 × 10-19 J

Question 14

Question

Predict the charge of the ion formed from: Al [blank_start]3+[blank_end] Na [blank_start]1+[blank_end] Br [blank_start]1-[blank_end] Mg [blank_start]2+[blank_end] N [blank_start]3-[blank_end] O [blank_start]2-[blank_end] Ne [blank_start]won’t form ion[blank_end]

Answer

3+
1+
1-
2+
3-
2-
won’t form ion

Question 15

Question

Predict the charge of the ion formed from: Al 3+ Na 1+ Br 1- Mg 2+ N 3- O 2- Ne won’t form ion Which of the above are metals? [blank_start]Al, Na, Mg[blank_end]

Answer

Al, Na, Mg

Question 16

Question

Write the electron configurations for: Se [blank_start]1s22s22p63s23p64s23d104p4[blank_end] Mn2+ [blank_start]1s22s22p63s23p64s03d5[blank_end] Fe2+ [blank_start]1s22s22p63s23p64s03d6[blank_end] S [blank_start]1s22s22p63s23p4[blank_end]

Answer

1s22s22p63s23p64s23d104p4
1s22s22p63s23p64s03d5
1s22s22p63s23p64s03d6
1s22s22p63s23p4

Question 17

Question

Give the number of core electrons and valence electrons for Se [blank_start]28/6[blank_end] and Sulfur [blank_start]10/6.[blank_end]

Answer

28/6
10/6

Question 18

Question

Write an orbital diagram for oxygen

Answer

True
False

Question 19

Question

No two electrons can have the same four quantum numbers is known as the

Answer

Pauli exclusion principle.
Hund's rule
Aufbau principle
Heisenberg uncertainty principle

Question 20

Question

Only two electrons, with opposing spins, are allowed in each orbital is known as the

Answer

Pauli exclusion principle
Hund's rule
Aufbau principle
Heisenberg uncertainty principle

Question 21

Question

When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as

Answer

Pauli exclusion principle
Hund's rule
Aufbau principle
Heisenberg uncertainty principle

Question 22

Question

Place the following elements in order of increasing atomic radius P Ba Cl

Answer

Ba < P < Cl
P < Cl < Ba
Cl < P < Ba
Cl < Ba < P
Ba < Cl < P

Question 23

Question

Place the following in order of increasing radius Br⁻ Na⁺ Rb⁺

Answer

Br⁻ < Rb⁺ < Na⁺
Na⁺ < Rb⁺ < Br⁻
Rb⁺ < Br⁻ < Na⁺
Br⁻ < Na⁺ < Rb⁺
Rb⁺ < Na⁺ < Br⁻

Question 24

Question

Write an reaction equation for the second electron affinity of oxygen

Answer

True
False

Question 25

Question

Write a reaction equation for the second ionization of magnesium

Answer

True
False

Question 26

Question

Place the following in order of increasing IE1. N F As

Answer

N < As < F
As < N < F
F < N < As
As < F < N
F < As < N

Question 27

Question

Place the following in order of decreasing metallic character.

Answer

P > As > K
As > P > K
K > P > As
As > K > P
K > As > P

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Final Exam 1-4

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Question 13

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	Created by Brian O'Neill over 7 years ago