WGU D425 INTRO TO CHEMISTRY
OBJECTIVE ASSESSMENT ACTUAL
EXAM 2025/2026 ACCURATE QUESTIONS
WITH CORRECT DETAILED ANSWERS ||
100% GUARANTEED PASS
<NEWEST VERSION>
1. What's a compound? - ANSWER ✓ A substance made up of 2 or more
different elements joined together.
2. What's an example of a compound? - ANSWER ✓ H2O, table salt
3. What is a mixture? - ANSWER ✓ A combination of 2 or more pure
substances that retains its own identity & properties.
4. What are the 2 types of Mixtures? - ANSWER ✓ homogeneous and
heterogeneous mixtures
5. What's an example of a mixture? - ANSWER ✓ Salt water
6. Can matter be a mixture or pure substance? - ANSWER ✓ Yes, it can be
both.
7. What is a homogeneous mixture? - ANSWER ✓ a mixture that is the same
throughout
8. What is a heterogeneous mixture? - ANSWER ✓ a mixture that is not
uniform throughout
,9. What is the difference between homogeneous mixture and a pure substance?
- ANSWER ✓ They both are uniformed, but the composition of pure
substance is always the same and in homogenous mixture each sample may
vary.
10.What's an example of a homogeneous mixture? - ANSWER ✓ air and salt
water
11.What's an example of heterogeneous? - ANSWER ✓ Veggie soup, water
and oil
12.What are the 2 types of pure substances? - ANSWER ✓ elements and
compounds
13.What is alloy? - ANSWER ✓ A mixture of 2 or more elements, at least one
is a metal.
14.What is an example of an alloy? - ANSWER ✓ Brass (copper & zinc),
bronze (copper & tin)
15.Comparing Q and K - ANSWER ✓ 1. K>Q, shifts right
2. Q=K, at equilibrium
3. K<Q, shifts left
16.Position of equilibrium (k) - ANSWER ✓ • K > 1 : Products are favored at
equilibrium (reaction lies to the right).
• K < 1 : Reactants are favored at equilibrium (reaction lies to the left).
• K \approx 1 : Significant amounts of both reactants and products are
present at equilibrium.
17.Ideal gas behavior - ANSWER ✓ high temperature and low pressure
18.Rules for significant figures in calculations - ANSWER ✓ 1. Addition or
Subtraction: The resulting value should be reported to the same number of
decimal places as that of the term with the least number of decimal places
, 2. Multiplication or Division: The resulting value should be reported to the
same number of significant figures as that of the term with the least number
of significant figures
% By Mass - ANSWER ✓ Mass percentage of a component in a mixture
g of part/ g of whole * 100%
19.% by Volume - ANSWER ✓ Volume percentage of a component in a
solution
formula: mL of part/mL of whole * 100
= mL of solute/mL of solute + solution *100
20.% by mass/volume - ANSWER ✓ Mass percentage of a solute in a volume
of solution
Formula: g of solute/mL of whole *100
21.Molarity - ANSWER ✓ Concentration of a solution in moles of solute per
liter of solution
mole of solute/total volume of solute+ mL of solvent
22.Dilution Formula - ANSWER ✓ C1V1 = C2V2; initial concentration x
initial volume = final concentration x final volume
23.Metric prefixes - ANSWER ✓ Units used to indicate multiples or fractions
of base units in the metric system
24.Density - ANSWER ✓ Mass per unit volume of a substance
Density=Mass/Volume
25.Average atomic mass - ANSWER ✓ Weighted average mass of isotopes of
an element
sum of all values(atomic mass of isootope * decimal abundance)
26.Calculate the density of 10.4mL sample of a substance with a mass of
35.12g. Enter the answer in the correct number of significant figures and
include the unit g/mL - ANSWER ✓
27.Convert 12.5g in to kilograms. enter answer in kg - ANSWER ✓ 0.0125
, 28.What defines a strong base - ANSWER ✓ a base that dissociates completely
in water. strong bases dissociate 100% in water to produce H+ ions
29.What is the definition of the equivalence point in titration - ANSWER ✓ the
point at which the amount of titrant added is just enough to completely
neutralize the analyte solution. Or measuring the volume of titrant solution
required for complete reaction with the analyte allows calculation of the
analyte concentration.
30.Octet rule - ANSWER ✓ States that atoms lose, gain or share electrons in
order to acquire a full set of eight valence electrons
31.Inert - ANSWER ✓ non reactive and generally do NOT form compounds
with other atoms because they are stable
32.Direct relationship - ANSWER ✓ a relationship in which one variable
increases with an increase in another variable
33.Inverse relationship - ANSWER ✓ a relationship in which one variable
decreases when another variable increases
34.Nobel Gases - ANSWER ✓ Atoms that have completely filled energy levels
or that eight electrons in their outermost energy level - do not easily lose
electrons. ( Group 8 or 18 )
35.Trigonal planar - ANSWER ✓ 3 bonds, 0 lone pairs. bonds have 120 degree
angles
36.Solute - ANSWER ✓ A substance in solution that is smaller than the
amount.
37.Physical state of a solution - ANSWER ✓ Describes how a mixture can be
classified, either solution, solvent, or solute.
38.Unsaturated solution - ANSWER ✓ A solution that has not yet reached its
maximum solubility.
39.Solution - ANSWER ✓ A homogeneous mixture of two or more substances.
OBJECTIVE ASSESSMENT ACTUAL
EXAM 2025/2026 ACCURATE QUESTIONS
WITH CORRECT DETAILED ANSWERS ||
100% GUARANTEED PASS
<NEWEST VERSION>
1. What's a compound? - ANSWER ✓ A substance made up of 2 or more
different elements joined together.
2. What's an example of a compound? - ANSWER ✓ H2O, table salt
3. What is a mixture? - ANSWER ✓ A combination of 2 or more pure
substances that retains its own identity & properties.
4. What are the 2 types of Mixtures? - ANSWER ✓ homogeneous and
heterogeneous mixtures
5. What's an example of a mixture? - ANSWER ✓ Salt water
6. Can matter be a mixture or pure substance? - ANSWER ✓ Yes, it can be
both.
7. What is a homogeneous mixture? - ANSWER ✓ a mixture that is the same
throughout
8. What is a heterogeneous mixture? - ANSWER ✓ a mixture that is not
uniform throughout
,9. What is the difference between homogeneous mixture and a pure substance?
- ANSWER ✓ They both are uniformed, but the composition of pure
substance is always the same and in homogenous mixture each sample may
vary.
10.What's an example of a homogeneous mixture? - ANSWER ✓ air and salt
water
11.What's an example of heterogeneous? - ANSWER ✓ Veggie soup, water
and oil
12.What are the 2 types of pure substances? - ANSWER ✓ elements and
compounds
13.What is alloy? - ANSWER ✓ A mixture of 2 or more elements, at least one
is a metal.
14.What is an example of an alloy? - ANSWER ✓ Brass (copper & zinc),
bronze (copper & tin)
15.Comparing Q and K - ANSWER ✓ 1. K>Q, shifts right
2. Q=K, at equilibrium
3. K<Q, shifts left
16.Position of equilibrium (k) - ANSWER ✓ • K > 1 : Products are favored at
equilibrium (reaction lies to the right).
• K < 1 : Reactants are favored at equilibrium (reaction lies to the left).
• K \approx 1 : Significant amounts of both reactants and products are
present at equilibrium.
17.Ideal gas behavior - ANSWER ✓ high temperature and low pressure
18.Rules for significant figures in calculations - ANSWER ✓ 1. Addition or
Subtraction: The resulting value should be reported to the same number of
decimal places as that of the term with the least number of decimal places
, 2. Multiplication or Division: The resulting value should be reported to the
same number of significant figures as that of the term with the least number
of significant figures
% By Mass - ANSWER ✓ Mass percentage of a component in a mixture
g of part/ g of whole * 100%
19.% by Volume - ANSWER ✓ Volume percentage of a component in a
solution
formula: mL of part/mL of whole * 100
= mL of solute/mL of solute + solution *100
20.% by mass/volume - ANSWER ✓ Mass percentage of a solute in a volume
of solution
Formula: g of solute/mL of whole *100
21.Molarity - ANSWER ✓ Concentration of a solution in moles of solute per
liter of solution
mole of solute/total volume of solute+ mL of solvent
22.Dilution Formula - ANSWER ✓ C1V1 = C2V2; initial concentration x
initial volume = final concentration x final volume
23.Metric prefixes - ANSWER ✓ Units used to indicate multiples or fractions
of base units in the metric system
24.Density - ANSWER ✓ Mass per unit volume of a substance
Density=Mass/Volume
25.Average atomic mass - ANSWER ✓ Weighted average mass of isotopes of
an element
sum of all values(atomic mass of isootope * decimal abundance)
26.Calculate the density of 10.4mL sample of a substance with a mass of
35.12g. Enter the answer in the correct number of significant figures and
include the unit g/mL - ANSWER ✓
27.Convert 12.5g in to kilograms. enter answer in kg - ANSWER ✓ 0.0125
, 28.What defines a strong base - ANSWER ✓ a base that dissociates completely
in water. strong bases dissociate 100% in water to produce H+ ions
29.What is the definition of the equivalence point in titration - ANSWER ✓ the
point at which the amount of titrant added is just enough to completely
neutralize the analyte solution. Or measuring the volume of titrant solution
required for complete reaction with the analyte allows calculation of the
analyte concentration.
30.Octet rule - ANSWER ✓ States that atoms lose, gain or share electrons in
order to acquire a full set of eight valence electrons
31.Inert - ANSWER ✓ non reactive and generally do NOT form compounds
with other atoms because they are stable
32.Direct relationship - ANSWER ✓ a relationship in which one variable
increases with an increase in another variable
33.Inverse relationship - ANSWER ✓ a relationship in which one variable
decreases when another variable increases
34.Nobel Gases - ANSWER ✓ Atoms that have completely filled energy levels
or that eight electrons in their outermost energy level - do not easily lose
electrons. ( Group 8 or 18 )
35.Trigonal planar - ANSWER ✓ 3 bonds, 0 lone pairs. bonds have 120 degree
angles
36.Solute - ANSWER ✓ A substance in solution that is smaller than the
amount.
37.Physical state of a solution - ANSWER ✓ Describes how a mixture can be
classified, either solution, solvent, or solute.
38.Unsaturated solution - ANSWER ✓ A solution that has not yet reached its
maximum solubility.
39.Solution - ANSWER ✓ A homogeneous mixture of two or more substances.
