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JHS Chemistry Final Exam Fall 2022

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Last updated about 3 years ago
65 questions
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Question 1
1.

If the temperature of a sample of gas is increased while maintaining constant pressure what happens to the volume?

Question 2
2.

If the temperature of a gas is kept constant, the pressure and volume of the gas are

Question 3
3.

Which of the following defines standard temperature?

Question 4
4.

Which of the following defines standard pressure?

Question 5
5.

Raising the temperature of a gas in a fixed volume container will most likely change the

Question 6
6.

The particles in a solid are

Question 7
7.

When the temperature decreases during a chemical reaction this described as a(n)________ reaction.

Question 8
8.

According to the kinetic-molecular theory, particles of matter are in constant motion in

Question 9
9.

Which set of characteristics correctly describes an ionic compound?

Question 10
10.

The origin of the word acid relates to how acids tend to taste, which is best described as

Question 11
11.

A smooth, slippery feel is associated with

Question 12
12.

What is the correct name of the acid HNO3?

Question 13
13.

The correct name of the acid HBr is

Question 14
14.

The pH of a basic solution is

Question 15
15.

Which of the following substances will NOT dissolve in water?

Question 16
16.

How does a covalent bond differ from an ionic bond?

Question 17
17.

Write out and balance the following chemical equation:
zinc reacts with iron (III) chloride yielding zinc chloride and iron

Question 18
18.

What is the name of the compound whose formula is (NH4)3PO4?

Question 19
19.

What is the name of the compound whose formula is FeSO4?

Question 20
20.

What is the name of the molecular substance PCl5?

Question 21
21.

In a reaction in which hydrogen reacts with oxygen to produce water, which substances are the reactants?

Question 22
22.

What is the molar mass of water?

Question 23
23.

How many total atoms are there in this expression 3Al2(SO4)3?

Question 24
24.

Which of the following is an empirical formula?

Question 25
25.

What is the formula (molar) mass of Ca(NO3)2?

Question 26
26.

The symbol (s) written after a formula in a chemical equation stands for

Question 27
27.

Two white powders are mixed in a flask. The bottom of the flask feels warmer. This is an example of what kind of reaction?

Question 28
28.

What number is represented by “∆” to balance the equation:  ∆Na + MgCl2 →  NaCl  +  Mg   ?

Question 29
29.

What will happen if a lead metal strip is placed into a solution of zinc nitrate? (hint: write out the equation first; what kind of reaction is it?)

Question 30
30.

Which of the following normally exists as a diatomic molecule?

Question 31
31.

What mass of phosphorous would be needed to produce 3.25 mol of P4O10 in the following reaction?
4 P (s) + 5 O2 (g) →   P4O10 (s)

Question 32
32.

How many grams of oxygen are required to react completely with 0.38 grams of hydrogen to form water?  __O2 + __H2 -> __H2O (hint: make sure it’s balanced!)

Question 33
33.

How many valence electrons does an element with an electron configuration of 1s22s22p63s23p5 have?

Question 34
34.

An atom will bond with another atom if both atoms have

Question 35
35.

In the reaction N2 +  3H2 →  2NH3, what is the mole ratio of nitrogen to ammonia?

Question 36
36.

The Haber process for producing ammonia commercially is represented by the equation:
N2 (g) + 3H2 (g) →  2NH3 (g)
To completely convert 9.0 mol hydrogen gas to NH3 gas, how many moles of nitrogen gas are required?

Question 37
37.

For the reaction  2Na +  2H2O  →  2NaOH  + H2, how many grams of sodium hydroxide are produced from 3.0 mol of water?

Question 38
38.

Valence electrons are those

Question 39
39.

The number of valence electrons that Group 15 elements have is

Question 40
40.

How many electrons does an atom of Magnesium that has a +2 charge have?

Question 41
41.

Name the compound N2O4.

Question 42
42.

How many neutrons does an average atom of Uranium have?

Question 43
43.

Which subatomic particle determines the identity of the atom?

Question 44
44.

What element has this noble gas electron configuration [Xe]6s2?

Question 45
45.

Elements in a group in the periodic table can be expected to have similar

Question 46
46.

What is the common charge for Nitrogen?

Question 47
47.

How many valence electrons does Chlorine have?

Question 48
48.

The molar mass of NH3 is 17.04 g/mol. How many moles of NH3 are present in 107.1 g?

Question 49
49.

What are the products of a combustion reaction?

Question 50
50.

Approved eye protection devices (such as goggles) are worn in the laboratory

Question 51
51.

Which of the following elements is a metalloid?

Question 52
52.

A sample of hydrogen gas had a volume of 455 L at 20°C and 755 mmHg. What would be its volume at 100°C and 565 mmHg?

Formula: P1V1 = P2V2
T1 T2

Question 53
53.

The pressure of a 250 mL sample of gas is 105 kPa. What would be the pressure if the volume was increased to 375 mL?

Formula: P1V1 = P2V2
T1 T2

Question 54
54.

What family does Bromine belong to?

Question 55
55.

What type of compound requires a roman numeral in its name?

Question 56
56.

A compound contains 32.38% sodium, 22.65% sulfur, and 44.99% oxygen. What is the empirical formula of the compound?

Question 57
57.

The molar mass of a carbon, hydrogen, and oxygen compound is 180 g/mol. If the empirical formula is CH2O, what is its molecular formula?

Question 58
58.

What is the percentage of calcium in calcium phosphide?

Question 59
59.

Which element is the only nonmetal located on the “metal side” of the periodic table?

Question 60
60.

The following data about a metal was collected in the lab. What is its density?

Question 61
61.

What type of reaction is this?
Ba(OH)2 → BaO + H2O

Question 62
62.

What type of reaction is this?
2Mg (s) + O2 (g) → 2MgO(s)

Question 63
63.

What type of reaction is this?
C3H8 + 5O2 → 3CO2 + 4H2O

Question 64
64.

What type of reaction is this?
Cl2 (g) + 2 KBr (aq) → 2KCl (aq) + Br2 (l)

Question 65
65.

What type of reaction is this?
Na2O + 2AgNO3 → 2NaNO3 + Ag2O