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Chem 1 Final > Comprehensive Makeup Exam > Flashcards

Comprehensive Makeup Exam Flashcards

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1
Q

Solids have a ____ shape and are not appreciably _______.

A

definite; compressible

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2
Q

If matter is uniform throughout, cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical process, it is called a(n) _______.

A

compound.

compound can only be separated by chemical process.
homogeneous mixture is easier to separate

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3
Q

A separation process that depends on differing abilities of substances to form gases is called _______.

A

distilation

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4
Q

The SI unit for mass is _______.

A

kilogram

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5
Q

Formula for density?

A

d= m/v

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6
Q

Elements in Group 6A are called?

A

chalcogens

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7
Q

Elements in Group 7A are called?

A

halogens

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8
Q

The formula of a salt is XCl₂. The X-ion in this salt has 28 electrons. The metal X is _____

A

Zn

Cl has a charge of -1 (times 2 for Cl₂) = -2
So X must have a +2 charge
Add 2 protons (aka atomic #)

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9
Q

The formula of ammonium carbonate is ________

A

(NH₄)₂CO₃

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10
Q

Molecular formula of heptane?

A

C₇H₁₆

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11
Q

What is the molecular formula for n-hexanol?

a) C₆H₁₂OH
b) C₆H₁₃OH
c) C₆H₁₄OH
d) C₇H₁₃OH
e) C₇H₁₄OH

A

C₆H₁₃OH

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12
Q

Convert 9.316 x 10⁻⁷m to nm

A

932 nm

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13
Q

What is the formula for wavelength?

A

c=λf

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14
Q

What is the speed of light? What is its variable?

A

c= 3x10⁸ m/s

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15
Q

What is the formula for energy?

A

E=hv

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16
Q

What is planck’s constant?

A

h= 6.626 x 10⁻³⁴

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17
Q

The wavelength of a photon that has an energy of 5.25 x 10⁻¹⁹J is ________ m

A

3.79 x 10⁻⁷

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18
Q

How many p-orbitals are occupied in a Ne atom?

A

3 p-orbitals – 1s²2s²2p⁶ – one p-subshell (3 orbitals per -subshell)

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19
Q

Each p-subshell has ___ p-orbitals

A

3

20
Q

Each p-subshell can accommodate a maximum of ______ electrons

A

6

The p-subshell has 3 p-orbitals, each of which holds a maximum of 2 electrons, giving a maximum of 6 electrons per p-subshell.

21
Q

Each s-subshell can accommodate a maximum of _____ electrons

A

2

22
Q

Each d-subshell can accommodate a maximum of _____ electrons

A

10

23
Q

Each d-subshell has ___ orbitals

A

5

24
Q

The electron configuration of a ground-state Ag atom is ________

A

Ag and Cu are an exceptions.

[Kr] 5s¹4d¹⁰

Kr = 36
Ag = 47
25
Q

What is the electron configuration for Se?

A

[Ar] 3d¹⁰4s²4p⁴

26
Q

A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula?

A

C₈H₈O₂

27
Q

A 22.5g sample of ammonium carbonate contains ________ mol of ammonium ions

A

0.468

(NH₄)₂CO₃ — Sub2 means TWO MOLES AMMONIUM

28
Q

When H₂SO₂ is neutralized by NaOH in aqueous solution, the net ionic equation is ________

A

H⁺ (aq) + OH⁻ (aq) –> H₂O (l)

29
Q

What are the spectator ions in the reaction between KOH (aq) and HNO₃ (aq)?

A

K⁺ and NO₃⁻

30
Q

What is the molarity formula? and the units?

A

M=moles/volume

molarity=moles/liters

31
Q

How many K⁺ moles are present in 343 mL of a 1.27 M solution of potassium phosphate?

A

1.31

32
Q

A 31.5 mL aliquot of H₂SO₄ (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was _______

A

0.0051

33
Q

Distillation formula?

A

M₁V₁=M₂V₂

34
Q

The reaction of 50 mL of N₂ gas with 150mL of H₂ gas to form ammonia will produce _______mL ammonia if pressure and temperature are constant

A

100

35
Q

What mass (g) of NaN₃ is required to provide 40.0 L of N₂ at 25.0⁰C and 763 torr?

2NaN₃ (s) –> 2Na (s) + 3N₂ (g)

A

71.7

36
Q

What is the conversion from atm to torr?

A

1 atm = 760 torr // 760 mmHg

37
Q

What volume (L) of NH₃ gas at STP is produced by the complete reaction of 7.5 g of H₂O according to the following reaction?

Mg₃N₂ (s) + 6H₂O (l) –> 3Mg(OH)₂ (aq) + 2NH₃ (g)

A

3.1

STP:
1 mol = 22.4 L
Pressure= 1 atm
Temperature = 273 K

38
Q

STP conditions?

A

Pressure= 1 atm
Temperature = 273 K
1 mol = 22.4 L

39
Q

An ideal gas differs from a real gas in that the molecules of an ideal gas _________

A

have no attraction for one another

40
Q

What is Charles’ Law?

A

V₁ V₂
—- = —-
T₁ T₂

41
Q

A 3.5 L Scuba tank at 33 C was filled from a 12.0 L nitrogen tank at 27 C and 1.25 atm and a 10.8 L oxygen tank at 23 C and 1.15 atm.

What is the total pressure in the tank?
Partial pressure of Nitrogen and Oxygen?

A

Total Pressure = 8.04 atm

Partial Pressure:
Nitrogen= 4.286
Oxygen= 3.55

42
Q

The energy of a photon that has a wavelength of 13.2 nm is _______ J

A

1.51 x 10⁻¹⁷ J

3x10⁸= (13.2 x 10⁻⁹)f
f=2.27 x 10¹⁶
E= (6.626 x 10⁻³⁴)(2.27 x 10¹⁶)
E=1.51 x 10⁻¹⁷ J

43
Q

What is the formula for the combined gas law?

A

V₁P₁ V₂P₂
——- = ——
n₁T₁ n₂T₂

44
Q

The pressure of a sample of CH₄ gas (6.022 g) in a 30.0 L vessel at 402 K is ______ atm.

A

0.413

45
Q

What elements are insoluble?

A

S // alkali metals, NH₄, Sr, Ba, Ca
OH // alkali metals, NH₄, Sr, Ba, Ca
CO₃ // alkali metals, NH₄
PO₄ // alkali metals, NH₄

46
Q

What elements are soluble?

A

NO₃⁻ and C₂H₃O₂ // always
Cl, Br, I // Ag, Hg, Pb
SO₄ // Sr, Ba, Ca

47
Q

Constant for R

A

0.0821

Chem 1 Final (2 decks)

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