Deck 1: The Nature of Chemistry

Question 1

Which of the following is both a quantitative and a qualitative statement?

A) The reaction produced 112 g of a pure white solid.
B) The compound has a mass of 14.62 g.
C) The compound formed pale yellow crystals.
D) The drug is 92.5% pure.
E) The compound melted.

Answer 1

The reaction produced 112 g of a pure white solid.

Question 2

Which of the following is not a physical property?

A) pressure
B) heat capacity
C) hardness
D) reactivity
E) temperature

Answer 2

reactivity

Question 3

Which of the following is not matter?

A) Bacteria.
B) Smoke.
C) Paper.
D) Emotions.
E) Both b and d.

Answer 3

Emotions.

Question 4

A comfortable room temperature is 72 °F. Correctly estimating this temperature in Celsius yields:

A) 8.0 °C.
B) 14 °C.
C) 22 °C.
D) 54 °C.
E) 98 °C.

Question 5

Which of the following does not describe a physical property?

A) Aluminum melts at 660°C.
B) Elemental sulfur appears yellow in color.
C) A lead brick sinks in water.
D) Paper burns to ash.
E) Table sugar often appears as granulated powder.

Question 6

A sample has a mass of 297 g and a volume of 33 cm³. What is the identity of the sample?

A) silver (density = 10.5 g/cm³)
B) iron (density = 7.86 g/cm³)
C) mercury (density = 13.6 g/cm³)
D) copper (density = 8.92 g/cm³)
E) aluminum (density = 2.7 g/cm³)

Question 7

Water is an unusual substance in that the density of the solid state (ice) is normally lower than the density of the liquid state. Suppose a friend brings you a glass of ice water. If you leave the glass untouched, what will happen over time?

A) The ice will melt and the resulting water level will be lower than before.
B) The ice will melt and the resulting water level will be unchanged.
C) The ice will melt and the resulting water level will be higher than before.
D) The ice will only melt if the mixture is stirred.
E) None of these.

Question 8

Which of the following is not a physical property of water?

A) Water is a liquid at room temperature.
B) Water is transparent to visible light.
C) Water boils at 100°C.
D) Water freezes at 32°F.
E) Water can be broken down into hydrogen gas and oxygen gas.

Question 9

On an average day in February, the temperature at noon in Wisconsin is most likely to be:

A) -30°C
B) 0°C
C) 30°C
D) 60°C
E) 100°C

Question 10

The freezing point and boiling point of water are often used to calibrate thermometers. Give those temperatures in degrees Celsius.

A) 0 and 100
B) 273 and 373
C) 32 and 212
D) 0 and 373
E) 100 and 273

Question 11

Table sugar melts at 366°F. Correctly estimating this temperature in Celsius yields:

A) 334°C
B) 221°C
C) 203°C
D) 186°C
E) 171°C

Question 12

A statement that includes a measurement or number is a:

A) model
B) law
C) quantitative statement
D) qualitative statement
E) hypothesis

Question 13

Which of the following is a qualitative statement?

A) The compound is contaminated.
B) The reactants are 99.95% pure.
C) The sample has a mass of 85 grams.
D) The reaction produced 112 g of a pure white solid.
E) The gas volume is twenty-two liters.

Question 14

What is a statement summarizing a group of scientific facts called?

A) law
B) theory
C) model
D) qualitative statement
E) hypothesis

Question 15

Which of the following is a chemical property of iron?

A) Iron conducts heat.
B) Iron conducts electricity.
C) Iron melts at 1535°C.
D) Iron can be bent into shapes.
E) Iron rusts on exposure to water and oxygen.

Question 16

What is a possible explanation of observations called?

A) law
B) model
C) qualitative statement
D) hypothesis
E) theory

Question 17

All of the following properties of a substance can aid in its identification except:

A) density.
B) temperature.
C) reactivity.
D) melting point.
E) boiling point.

Question 18

A unifying principle that explains a body of facts is a:

A) model.
B) law.
C) qualitative statement.
D) hypothesis.
E) theory.

Question 19

A sample of gold has a mass of 63.49 g. What is its volume? (Density of gold = 19.3 g/mL)

A) 1225 mL
B) 63.5 mL
C) 44.2 mL
D) 3.29 mL
E) 0.304 mL

Question 20

A sample has a mass of 612 g and a volume of 78 cm³. What is the identity of the sample?

A) mercury (density = 13.6 g/cm³)
B) iron (density = 7.86 g/cm³)
C) copper (density = 8.92 g/cm³)
D) silver (density = 10.5 g/cm³)
E) aluminum (density = 2.7 g/cm³)

Question 21

Which of the following is not part of Dalton's Atomic Theory?

A) Matter is not created nor destroyed in a chemical reaction; the molecular arrangements are changed.
B) An atom of one element can be chemically transformed into a different type of atom.
C) Atoms of different elements combine in whole number quantities.
D) Atoms of a given element have the same mass.
E) Atoms of different elements have different masses.

Question 22

Which of the following does not occur when ice melts?

A) Its molecular composition changes.
B) The arrangement of molecules changes.
C) The speed of the molecules changes.
D) Its density changes.
E) Its shape changes.

Question 23

Which of the following describes a chemical change?

A) Shredding paper.
B) Whipping cream.
C) Grinding coffee beans.
D) Crushing an aluminum can.
E) Burning wood.

Question 24

Which of the following will not have a specific composition and specific properties?

A) ozone
B) water
C) ammonia
D) steel
E) aspirin

Question 25

Aluminum, salt, and coffee are:

A) an element, a homogeneous mixture, and a pure substance.
B) a pure substance, a heterogeneous mixture, and a pure substance.
C) a homogeneous mixture, a pure substance, and a homogeneous mixture.
D) an element, a pure substance, and a homogeneous mixture.
E) none of these.

Question 26

Which is the best definition of a pure substance?

A) A material that contains two or more types of atoms
B) A material in the gas phase
C) A material whose properties cannot be changed by further physical separation
D) A material whose properties have been measured
E) A material that has been heated

Question 27

Which of the following is not a chemical property of water?

A) Water interacts with some metals to produce hydrogen gas.
B) Water combines with carbon dioxide in plants to produce starches and sugars.
C) Water boils at 100 degrees Celsius.
D) Water combines with sulfur dioxide and oxygen to produce sulfuric acid.
E) Water and carbon dioxide are produced by the combustion of fossil fuels.

Question 28

Which of the following would not convert a heterogeneous mixture into a more homogeneous material?

A) filtering a salt solution
B) magnetically removing iron from an iron-sulfur mixture
C) filtering sand away from water
D) picking rice grains from a mixture of rice and peas
E) doing chromatography on an ink sample

Question 29

According to the Kinetic Molecular Theory, as the temperature of a compound increases:

A) its molecular motion increases
B) its melting point increases
C) it freezes
D) its boiling point increases
E) all of these

Question 30

Which characteristics apply to the gaseous state?
I. low density
II. high density
III. rapid molecular motion
IV. slow molecular motion
V. large distance between particles

A) I, V
B) II, V
C) II, III, V
D) I, IV, V
E) I, III, V

Question 31

Which of the following is heterogeneous?

A) black coffee
B) copper pipe
C) a clear sugar solution
D) grape juice
E) a tossed salad

Question 32

Which of the following describes a chemical change?

A) Ethanol is a clear, colorless liquid.
B) Ethanol can be produced by the fermentation of grapes.
C) Ethanol evaporates quickly at room temperature.
D) Ethanol has a high heat capacity.
E) Ethanol boils when heated.

Question 33

Which characteristic below best fits the description of a solid?

A) large distances between the molecules
B) molecules that are close together but are moving past one another
C) highly disordered molecules
D) rapid molecular motion
E) highly ordered molecules

Question 34

Which characteristic below best fits the description of a liquid?

A) rapid molecular motion
B) highly disordered molecules
C) large distances between the molecules
D) molecules that are close together but are moving past one another
E) highly ordered molecules

Question 35

Which of the following is not a solution?

A) red wine
B) alcohol in water
C) brass
D) air
E) ice in water

Question 36

Three length scales ordered from smallest to largest are:

A) microscale, nanoscale, macroscale.
B) microscale, macroscale, nanoscale.
C) macroscale, nanoscale, microscale.
D) nanoscale, microscale, macroscale.
E) none of these.

Question 37

Which of the following is not part of Dalton's Atomic Theory?

A) Atoms of the same element have the same mass and properties.
B) Different elements have atoms that are different from one another.
C) Atoms can combine in fractional numbers.
D) Atoms are indestructible.
E) All matter is made up of atoms.

Question 38

Bacteria, sugar molecules, and water droplets are matter at the:

A) microscale, nanoscale, macroscale.
B) microscale, macroscale, nanoscale.
C) macroscale, nanoscale, microscale.
D) nanoscale, microscale, macroscale.
E) none of these.

Question 39

Which of the following substances is homogeneous?

A) wood
B) a jelly bean
C) vegetable soup
D) salt dissolved in water
E) a mirror

Question 40

Which state of matter has no definite shape:

A) solid
B) liquid
C) gas
D) b and c
E) all of these

Question 41

A mixture that is nonuniform in composition is a(n) _____________ mixture.

Question 42

Which of the following is not a metal?

A) nickel (Ni, atomic number 28)
B) sulfur (S, atomic number 16)
C) lithium (Li, atomic number 3)
D) uranium (U, atomic number 92)
E) calcium (Ca, atomic number 20)

Question 43

Which of the following represents a pair of allotropes?

A) air and oxygen
B) glucose and sucrose
C) graphite and diamond
D) sand and glass
E) carbon monoxide and carbon dioxide

Question 44

How many of each type of atoms does the compound Cs₂SO₄ contain?

A) 2 cesium, 1 sulfur and 4 oxygen
B) 2 cesium, 1 silicon and 4 oxygen
C) 2 cesium, 1 selenium and 4 oxygen
D) 2 cerium, 1 sulfur and 4 oxygen
E) 2 cerium, 3 silicon and 4 oxygen

Question 45

Which of the following is a metal?

A) helium (He, atomic number 2)
B) nitrogen (N, atomic number 7)
C) sodium (Na, atomic number 11)
D) selenium (Se, atomic number 34)
E) carbon (C, atomic number 6)

Question 46

An element which has some properties of metals and some properties of nonmetals is called a(n) _____________.

Question 47

Water droplets, water molecules, and H₂O are water at the following levels:

A) symbolic, nanoscale, macroscale.
B) macroscale, symbolic, nanoscale.
C) macroscale, nanoscale, symbolic.
D) nanoscale, symbolic, macroscale.
E) nanoscale, macroscale, symbolic.

Question 48

Which of the following is not the symbol of an element?

A) Cu
B) Ni
C) CO
D) Ag
E) C

Question 49

Which of the following is a metalloid?

A) silicon (Si, atomic number 14)
B) hydrogen (H, atomic number 1)
C) tungsten (W, atomic number 74)
D) chlorine (Cl, atomic number 17)
E) uranium (U, atomic number 92)

Question 50

Combining two hydrogen atoms with one oxygen atom yields water while combining two hydrogen atoms with two oxygen atoms yields hydrogen peroxide. This is an example of:

A) The Law of Conservation of Mass.
B) Dalton's Atomic Theory.
C) The Law of Constant Composition.
D) The Law of Multiple Proportion.
E) The Law of Conservation of Energy.

Question 51

Ethanol contains 2 carbons, 6 hydrogens, 1 oxygen. Write its chemical formula.

Question 52

Burning of hydrogen fuel is a(n) _____________ change.

Question 53

In a chemical reaction, 36 g of water is broken down to yield 32 g of oxygen gas and 4 g of hydrogen gas. This is an example of:

A) The Law of Constant Composition.
B) The Law of Multiple Proportion .
C) The Law of Conservation of Energy.
D) The Law of Conservation of Mass.
E) Dalton's Atomic Theory.

Question 54

Hydrogen peroxide contains 2 hydrogens and 2 oxygens. Write its chemical formula.

Question 55

In a chemical reaction, 23.2 g of mercury oxide is broken down to yield 20 g of mercury and 3.2 g of oxygen gas. This is an example of:

A) The Law of Conservation of Mass.
B) The Law of Multiple Proportion.
C) The Law of Conservation of Energy.
D) Dalton's Atomic Theory.
E) The Law of Constant Composition.

Question 56

Carbon dioxide is always composed of three parts by weight of carbon and eight parts by weight of oxygen. This is an example of:

A) Dalton's Atomic Theory.
B) The Law of Constant Composition.
C) The Law of Conservation of Energy.
D) The Law of Conservation of Mass.
E) The Law of Multiple Proportion.

Question 57

A substance's melting point is an example of a(n) _____________ property.

Question 58

Which of the following is not the symbol of an element?

A) At
B) Kr
C) Fr
D) Os
E) Rx

Question 59

How many of each type of atoms does the compound mercury acetate, FePO₄ contain?

A) 1 francium, 1 potassium, 4 oxygen
B) 1 francium, 1 phosphorus, 4 oxygen
C) 1 francium, 1 polonium, 4 oxygen
D) 1 iron, 1 potassium, 4 oxygen
E) 1 iron, 1 phosphorus, 4 oxygen

Question 60

Methane is always composed of three parts by weight of carbon and one part by weight of hydrogen. This is an example of:

A) The Law of Conservation of Mass.
B) Dalton's Atomic Theory.
C) The Law of Constant Composition.
D) The Law of Multiple Proportion.
E) The Law of Conservation of Energy.

Question 62

The ability to conduct electricity is a(n) _____________ property.

Question 63

Filtering impurities out of water is a(n) _____________ process.

Question 64

Which state of matter is characterized by a variable shape but not volume?

Question 65

Oxygen (O₂) and ozone (O₃) are _____________ of the same element.

Question 66

How many atoms are in a diatomic molecule?.

Question 67

Color is a(n) _____________ property.

Question 68

The energy is the capacity to do _____________.

Question 69

Match the following: