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Final Exam Flashcards

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1
Q

Express 0.0000000789 in scientific notation using the correct number of sig figs.

A) 7.89 E -7

B) 7.89 E 8

C) 7.89 E 7

D) 7.89 E -8

A

7.89 E -8

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2
Q

Write 6.83 E 5 using correct scientific notation

A) 0.0000683

B) 683000

C) 6.83000

D) 6.00083

A

683000

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3
Q

A significant figure is

A) every digit in a measurement that is known with certainty plus two uncertain digits.

B) every digit in a measurement that is known with certainty.

C) every digit in a measurement that is known with certainty plus one uncertain.

D) every digit in a measurement that is known with certainty plus every uncertain digit.

A

Every digit in a measurement that is known plus every uncertain digit

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4
Q

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

A) tarnishing of copper

B) density

C) characteristic color

D) electrical conductivity

A

Tarnishing of copper

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5
Q

A(n) ________ is a tentative, testable explanation based on observations.

A) conclusion

B) hypothesis

C) experiment

D) law

A

Hypothesis

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6
Q

Which of the following is a chemical change?

A) decaying banana

B) boiling of water

C) sanding wood

D) carving a piece of marble

A

Decaying banana

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7
Q

Which of the following has been thoroughly tested and explains the results of many experiments?

A) theory

B) conclusion

C) hypothesis

D) law

A

Theory

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8
Q

Which of the following is NOT a physical property?

A) flammability

B) state of matter

C) texture

D) density

A

Flammability

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9
Q

Which of the following best describes the difference between a physical and chemical property?

A) Physical properties describe the appearance of a substance whereas chemical properties describe how the chemical structure of a substance may be changed.

B) Physical properties can always be observed with the eye whereas chemical properties must be measured microscopically.

C) Physical properties are based on matter whereas chemical properties are based on energy.

D) Chemical properties describe the appearance of a substance whereas physical properties describe how the chemical structure of a substance may be changed.

A

Physical properties describe the appearance of a substance whereas chemical properties describe how the chemical structure of a substance may be changed.

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10
Q

Which lists in the correct order, the steps of the scientific method?

A) make observations, experiment, form hypothesis, results, identify problem

B) experiment, make observations, identify problem, results, form hypothesis

C) form hypothesis, make observations, identify problem, experiment, results

D) Identify problem, make observations, form hypothesis, experiment, results

A

Identify problem, make observations, form hypothesis, experiment, results

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11
Q

_______________ is the science that studies matter, its composition and structure, and the changes it undergoes.

A) A physical property

B) The scientific method

C) Chemistry

D) Density

A

Chemistry

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12
Q

In one second, light travels 2.998 × 108 meters. Which of the following is the correct way to write this in conventional notation?

A) none of these

B) 299,800,000 m/s

C) 0.00000002998 m/s

D) 2,998,000 m/s

A

299,800,000 m/s

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12
Q

Which of the following is the correct order of lengths?

A) mm > cm > m > km

B) cm > km > nm > mm

C) mm > m > cm > km

D) km > cm > mm > μm

A

km > cm > mm > μm

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13
Q

Nanoparticles have an approximate length of 0.1 × 10–10 meters. Which of the following is the correct way to write this in conventional notation?

A) 0.00000000001 m

B) 10,000,000 m

C) 0.000000001 m

D) 1,000,000,000 m

A

A) 0.00000000001 m

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14
Q

Daytime temperatures in a desert can reach 50.0°C. What is this temperature on the Fahrenheit temperature scale?

A

(C x 9/5) + 32 = F

122.0 F

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15
Q

Which of the following is the largest number?

A) 5 × 10 4

B) 3.5 × 10–6

C) 3 × 10 3

D) 3 × 10–2

A

5 x 10 4

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15
Q

A patient is admitted to the hospital. She weighs 186 lb. She is to receive an IV medication based on her body weight. The physician’s order reads: give 2.0 mg per kg. The label on the medication reads 10. mg per mL. Calculate how many mL of this medication you would administer to this patient.

A

Convert the patient’s weight from pounds to kilograms:
186 lb * (1 kg / 2.20462 lb) ≈ 84.37 kg
Determine the total dosage required:
84.37 kg * 2.0 mg/kg = 168.74 mg
Calculate the volume of medication needed based on the concentration provided on the label:
Concentration: 10 mg/mL
Volume (mL) = Total dosage (mg) / Concentration (mg/mL)
= 168.74 mg / 10 mg/mL
≈ 16.874 mL

16.9 mL

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16
Q

The metric prefix that means 1000 times larger is ________________.

A

Kilo

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17
Q

The boiling point of liquid oxygen is 90.2 K. What is this temperature on the Celsius scale?

A

K - 273.15 = C

-182.8 C

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18
Q

Convert 40.2 space degree C to Kelvin. (Round your answer to the tenths place- that is, one place past the decimal.)

A

C+ 273.15 = K

313.4 K

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19
Q

When solving problems using dimensional analysis, always start with the ________.

A

Given

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20
Q

_____________________ uses units to solve problems.

A

Dimensional Analysis

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20
Q

Choose which of the following conversion factors is incorrect.

A) 1000 km = 1 meter

B) 1000 mL = 1 L

C) 1000000 mcg = 1 g

D) 1000000 games = 1 Mgame

A

1000 km = 1 Meter

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21
Q

Children’s chewable acetamenophen contains 75 mg of acetamenophen per tablet. If the recommended dosage for this medication is 10. mg/ kg, how many tablets should you give to a child who weighs 52 pounds? Because this is a tablet, round the answer to the nearest whole number

A

Convert the child’s weight from pounds to kilograms:
52 lb * (1 kg / 2.20462 lb) ≈ 23.59 kg
Determine the total dosage required based on the weight:
Total dosage = Weight (kg) * Dosage per kg
= 23.59 kg * 10 mg/kg
= 235.9 mg
Divide the total dosage required by the dosage per tablet:
Number of tablets = Total dosage / Dosage per tablet
= 235.9 mg / 75 mg/tablet
≈ 3.15

3 Tabs

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22
Q

The boiling point of methanol is 65°C. What is this temperature on the Fahrenheit scale?

A

(C x 9/5) + 32

149 F

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23
Q

Do this problem using dimensional analysis. Make sure to round your answers appropriately.

Calculate the number of km there are in 1.1 miles.

A

1.1 miles×
1 mile
1.60934 kilometers
​
=1.1×1.60934 kilometers

Now, we multiply the given value (1.1 miles) by the conversion factor:

1.1
×
1.60934
≈
1.77
kilometers
1.1×1.60934≈1.77 kilometers

Therefore, there are approximately 1.77 kilometers in 1.1 miles.

1.8 km

1.8 km

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24
Q

How many minutes are there in a 24-hour day? (Assume exactly 24 hours in a day.)

A

1.44 x 10 3

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25
Q

If gasoline costs $3.79 per gallon, what is the cost of 1.00 liter? [1 quart = 0.946 liter]

A

$1

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26
Q

In one second, light travels 2.998 × 108 meters. Which of the following is the correct way to write this in conventional notation?

A) none of these

B) 299,800,000 m/s

C) 0.00000002998 m/s

D) 2,998,000 m/s

A

299,800,000 m/s

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27
Q

_________ measures the average kinetic energy of the particles in a substance. In other words, how fast the particles are moving.

A

Temperature

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28
Q

The boiling point of liquid nitrogen is -195.8 °C. What is this temperature in Kelvins?

A

C+ 273.15 = K

77.35 K

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29
Q

________________ determines the state of matter.

A

Temperature

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30
Q

In which state of matter are the particles so tightly packed that they cannot change their position?

A

Solid

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31
Q

Which state of matter has the same volume but takes its shape of its container?

A

Liquid

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32
Q

Which of the following is true of ice, water, and steam?

A) They are three different chemical substances.

B) They are the same substance in different chemical states.

C) They are the same substance in different physical states.

D) They are the same substance in different chemical and physical states.

A

They are the same substance but in different physical states

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33
Q

In which state of matter are the particles farthest apart?

A

Gas

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34
Q

________________________ is defined as the weighted average of all the isotopes of an element.

A

Atomic Mass

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35
Q

Almost all of the mass of an atom is concentrated in the ________.

A

Nucleus

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36
Q

Almost all of the volume of an atom is found in the ________.

A

Energy levels

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37
Q

What is the correct isotopic symbol for an element that has a mass number of 48 and an atomic number of 22?

A

The atomic number (number of protons) is represented as a subscript on the left side of the element symbol.
The mass number (number of protons and neutrons combined) is represented as a superscript on the left side of the element symbol.

48
Ti
22

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38
Q

Which of the following is NOT a property of mixtures?

A) they can be separated by physical means

B) they are pure

C) they have definite composistion

D) the components lose their properties when mixed together

A

They are pure

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39
Q

A solution is another name for a(n) ___________________.

A

Homogeneous Mixture

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40
Q

Zinc can be mixed in differing amounts with copper to form an alloy called brass. What is brass an example of?

A

a homogeneous mixture

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41
Q

Who is credited with first discovering what he called an atom in the early 1800s?

A

John Dalton

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42
Q

____________________ are atoms of the same element with different numbers of neutrons.

A

isotopes

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42
Q

_____________________ is credited with putting together the first “modern” periodic table.

A

Dmitri Mendeleev

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43
Q

The __________________ tells the number of protons in an atom.

A

Atomic Number

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44
Q

The __________________ tells the number of protons plus neutrons in an atom.

A

mass number

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45
Q

The subatomic particle most responsible for giving an atom its behavior is the ________.

A

electron

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46
Q

The subatomic particle most responsible for holding the nucleus tightly bound together is the ___________.

A

Neutron

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47
Q

The subatomic particle most responsible for holding the nucleus tightly bound together is the ___________.

A

Neutrons

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48
Q

The unit used to measure the mass of a single atom (or particle in an atom) is the _______________.

A

atomic mass unit

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49
Q

With the exception of helium (He), all of the noble gases have electron configurations ending in

A

p^6

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50
Q

What are the horizontal rows of the periodic table called?

A

periods

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51
Q

____________________ have the properties of both metals and nonmetals.

A

metalloids

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52
Q

Of the elements listed below, which is/are a metal(s)?

Strontium (Sr), silicon (Si), sulfur (S), iodine (I), cesium (Cs)

A

Sr and Cs

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53
Q

___________________ are those found in the outer-most (highest) energy level.

A

Valence electrons

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54
Q

Which of the following columns of the periodic table contains only gaseous elements?

A) 8A

B) 6A

C) 7A

D) 5A

A

8A

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55
Q

Which of the following contains only nonmetals?

A) P, B, Si, and Na

B) C, Si, B, and Be

C) F, Cl, He, and C

D) none of these

A

F, Cl, He, and C

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56
Q

Which of the following places the elements in the correct order from smallest to largest?

A) Be < Ca < Ba < Ra

B) Ca < Ba < Be < Ra

C) Ra < Ba < Ca < Be

D) Ba < Ra < Ca < Be

A

Be < Ca < Ba < Ra

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57
Q

In every energy level beginning with the ______ there are _______ p-orbital(s).

A

2nd - 3

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58
Q

Which of the following places the elements in the correct order from smallest to largest?

A) Mg < K< Ca < Cl

B) K < Cl < P < Mg

C) P < Mg < K < Cl

D) Cl < P < Mg < K

A

Cl < P < Mg < K

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59
Q

A(n) ____________________ is a cloud shape formed when an electron is moving around the nucleus.

A

Orbital

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59
Q

What are the vertical columns of the periodic table called?

A

families

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60
Q

Match the letter to the family

A

A) Inner transition metals
B) Noble gas
C) Alkali metals
D) transition metals
E) halogens
F) Alkaline earth metals

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61
Q

Which is most likely true of an atom with six valence electrons?

A) It will gain one electron.

B) It will gain two electrons.

C) It will lose one electron.

D) It will lose two electrons.

A

it will gain 2 electrons

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62
Q

How many main types of chemical bonds exist?

A

2

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63
Q

Which of the following is true in general of all cations?

A) A cation has an equal number of protons and electrons.

B) A cation has fewer protons than electrons.

C) A cation has more protons than electrons.

D) A cation has more protons than neutrons.

A

a cation has more protons than electrons

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64
Q

Which of the following is generally true of all anions?

A) An anion has an equal number of protons and electrons.

B) An anion has fewer protons than electrons.

C) An anion has more protons than electrons.

D) An anion has more electrons than neutrons.

A

an anion has fewer protons than electrons

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65
Q

What is likely true of an atom with one valence electron?

A

it will lose an electron

66
Q

Which of the following elements is the most likely to lose electrons to become a cation?

A) Ar

B) S

C) I

D) Mg

A

Mg

67
Q

Which of the following ions has the same electronic configuration as argon?

A) K+

B) Ca2+

C) both K+ and Ca2+

D) neither K+ or Ca2+

A

both K+ or Ca2+

68
Q

In what form is lithium administered when it is used as a drug in the treatment of manic depression?

A

Li+

69
Q

What is the name of the species formed when a chlorine atom gains an electron?

A

Chloride Ion

70
Q

What is the valence shell electron configuration of all the noble gases except helium?

A

ns2np6

71
Q

Which of the following occurs when a calcium atom is converted to Ca2+?

A) The calcium atom gains two electrons and loses two protons.

B) The calcium atom gains two electrons.

C) The calcium atom loses two electrons and two protons.

D) The calcium atom loses two electrons.

A

The calcium atom loses two electrons

72
Q

What is the difference between a monatomic element and a diatomic element?

A

A monatomic element can be found uncombined in nature but a diatomic element will always be found in pairs.

73
Q

Which of the following atoms is the least likely to form an ion?

A) chlorine

B) potassium

C) xenon

D) iron

A

xenon

73
Q

Which of the following is NOT one of the diatomic elements?

A) He

B) H

C) O

D) Br

A

He

74
Q

What is the common name of Cu2+?

A

copper (II) ion

75
Q

the name for iron (III) ion?

A

Fe3+

76
Q

What is true of polyatomic ions?

A

The vast majority of polyatomic ions are anions.

77
Q

The “ide” ending is usually, but not always, associated with monatomic anions. Which of the following polyatomic ions has a name that ends in “ide”?

A) C2H3O2-

B) HPO42-

C) OH-

D) SO42-

A

OH-

78
Q

An ionic bond is associated with which of the following?

A) interactions between nuclei

B) equal sharing of electrons

C) unequal sharing of electrons

D) the transfer of electrons

A

the transfer of electrons

79
Q

Which of the following is true of ionic compounds?

A) They are liquids at room temperature.

B) They are gases in which individual molecules are present.

C) They are solids in which both cations and anions are present.

D) They share their electrons equally.

A

They are solids in which both cations and anions are present

80
Q

One common element used for embalming is sodium nitrate. What is the correct formula for sodium nitrate?

A

NaNo3

81
Q

AgCl is a chemical commonly used in photography. What is the correct name of AgCl?

A

Silver Chloride

82
Q

A compound used in the treatment of gout and manic depression has the formula Li2CO3. What is the name of this compound?

A

lithium carbonate

83
Q

A tin compound used for electroplating steel has the formula SnCl2. What is the systematic name of this compound?

A

tin (II) chloride

84
Q

The formula of a compound was found to be Fe2O3. What is the systematic name of this compound?

A

iron (III) oxide

85
Q

What is the correct formula of sodium fluoride?

A

NaF

86
Q

The term “limelight” is derived from the old name of calcium oxide. What is the formula of calcium oxide?

A

CaO

87
Q

What is the correct formula of aluminum oxide?

A

AI2O3

88
Q

What is the correct name of Al2(SO4)3?

A

aluminum sulfate

89
Q

What is the correct name of BaI2?

A

barium iodide

90
Q

What is the correct name of NH4NO3, a compound found in fertilizers?

A

ammonium nitrate

91
Q

What is the correct way to write the formula of the compound formed by a calcium ion and a sulfate ion?

A

CaSO4

92
Q

What the correct name and formula for the acid formed from hydrogen and chlorine?

A

Hydrochloric acid, HCI2

93
Q

A covalent bond is associated with

A

the sharing of electrons

94
Q

Laughing gas, sometimes called nitrous oxide, has the formula N2O. What is the proper chemical name of nitrous oxide?

A

dinitrogen monoxide

95
Q

What is the correct chemical name of a compound with the formula N2O3?

A

dinitrogen trioxide

96
Q

Though it is very rare, some noble gases will form a covalent compound. What is the correct name of XeF4?

A

xenon tetrafluoride

97
Q

What is the systematic name of CS2?

A

carbon disulfide

98
Q

Which types of elements generally have high electronegativities?

A

halogens

99
Q

What is the correct formula of dinitrogen pentoxide?

A

N2O5

100
Q

Which of the following is a triprotic acid?

A) HCl

B) HNO3

C) H2SO4

D) H3PO4

A

H3PO4

101
Q

The key to recognizing a decomposition reaction is

A

it only has one reactant

102
Q

The key to recognizing a synthesis reaction is

A

it only has one product

103
Q

The reaction 2KClO3(s) → KCl(s) + 3O2(g) is an example of a reaction.

A

decomposition

104
Q

The reaction 2CO + O2 → 2CO2 is an example of a ____________ reaction.

A

synthesis

105
Q

In a chemical equation, the _____________ are to the left of the arrow and the ______________ are to the right of the arrow.

A

reactants, products

106
Q

A(n) ________________________________ uses symbols and formulas to represent a chemical change.

A

chemical equation

107
Q

This is used to show the reactants or products are dissolved in water.

A

(aq)

108
Q

A _______________ separates two reactants or two products in a chemical equation.

A

+

109
Q

In order for a single replacement reaction to occur,

A

the single element must be higher on the Activity Series than the element in the compound that it would replace

110
Q

The key to recognizing a single replacement reaction is

A

it has one element and one compound on both sides.

111
Q

The reaction Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)
is an example of a _____________reaction.

A

single replacement

112
Q

The reaction BaCl2 + K2CO3 → BaCO3 + 2KCl is an example of a ______________ reaction.

A

double replacement

113
Q

One of the reactants in a combustion reaction must always be ______.

A

oxygen

114
Q

The key to recognizing a combustion reaction is

A

it has a hydrocarbon and oxygen as reactants.

115
Q

The products of a combustion reaction are

A

carbon dioxide and water

116
Q

The reaction CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
is an example of a _____________reaction.

A

combustion

117
Q

What is the correct set of integer coefficients for the balanced equation?

___C5H12(g) + ___O2(g) → ___CO2(g) + ___H2O(g)

A

1, 8, 5, 6

118
Q

What are the coefficients for the balanced equation?

___N + ____H2O —> NaOH___H2

A

2, 2, 2, 1

119
Q

___KNO3 + ___H2CO3___—> K2CO3___+ HNO3

A

2, 1, 1, 2

120
Q

___Al+___H2SO4 —> ___Al2 (SO4) 3 + H2

A

2, 3, 1, 3

121
Q

The reaction of nitric acid, HNO3(aq), with calcium carbonate, CaCO3(s), produces calcium nitrate, carbon dioxide, and water. Which of the following is the correct balanced equation for this reaction?

A

2HNO3(aq) + CaCO3(s) → Ca(NO3)2(aq) + CO2(g) + H2O(l)

121
Q

___C3H8(g) + ___O2(g) → ___CO2(g) + ___H2O(g)

A

1, 5, 3, 4

122
Q

Which of the following compounds is insoluble in water?

A) CaCO3

B) CaCl2

C) Ca(NO3)2

D) Ca(C2H3O2)2

A

CaCO3

123
Q

The products of the reaction of phosphoric acid, H3PO4(aq), and solid magnesium hydroxide, Mg(OH)2(s), are aqueous magnesium phosphate and water. What is the balanced equation for this reaction?

A

2H3PO4(aq) + 3Mg(OH)2(s) → Mg3(PO4)2(aq) + 6H2O(l)

124
Q

it is a photograph of a beaker containing a clear liquid. Another liquid is being poured from a test tube into the beaker. An insoluble white substance is being formed in the beaker.

Which of the following is most likely occurring in the beaker?

A

a precipitate forming

125
Q

What ion does an acid produce according to the original Arrhenius definition of an acid?

A

H+

126
Q

What ion does a base produce according to the original Arrhenius definition of a base?

A

OH-

127
Q

the correct name for the ion H3O+?

A

hydronium ion

128
Q

Which of the following can be characterized as a strong acid?

A) H3BO3

B) HCl

C) both H3BO3 and HCI

D) neither H3BO3 or HCI

A

HCI

129
Q

Which of the following occurs when NaOH is dissolved in water to form a basic solution?

A) A complex between NaOH and Cl is formed.

B) NaOH breaks up to form Na+(aq), H+(aq), and O2−(aq).

C) NaOH breaks up to form Na+(aq) and OH−(aq).

D) The water molecule loses an H+.

A

NaOH breaks up to form Na+(aq) and OH−(aq).

129
Q

Which of the following can be characterized as a strong base?

A) Ba(OH)2

B) NH3

C) both Ba(OH)2 and NH3

D) neither Ba(OH)2 or NH3

A

Ba(OH)2

130
Q

Which of the following acids is found in gastric fluid?

A) acetic

B) hydrochloric

C) nitric

D) sulfuric

A

hydrochloric

131
Q

What is the name of the acid that dissociates to give the nitrate ion, NO3−?

A

nitric acid

132
Q

What is the reaction between an acid and a base known as?

A

neutralization

133
Q

Which of the following pH values corresponds to a highly acidic solution?

A) 2.8

B) 6.8

C) 7.2

D) 11.2

A

2.8

134
Q

Which of the following pH values corresponds to a highly basic solution?

A) 2.8

B) 6.8

C) 7.2

D) 11.2

A

11.2

135
Q

It is a photograph of a pH meter measuring the pH of a clear liquid in a beaker. The meter reads 4.33.

How would the solution in the beaker be classified?

A

acidic

136
Q

The subatomic particle which establishes the identity of an element is the ____

A

Proton

137
Q

The number of neutrons in an atom can be found by

A

Subtracting the atomic number from the mass number

138
Q

What Greek philosopher is most closely associated with the concept of an atom

A

Aristotle

139
Q

What is not a property of mixtures

A

They can be separated by physical means

140
Q

The two main classes of matter are

A

Substances and mixtures

141
Q

____are located along the zig zag or stair step line on the periodic table

A

Metalloids

142
Q

Which state of matter is highly compressible

A

Gas

143
Q

What are the elements in the B column called

A

Main Group Elements

144
Q

What is true of ionic compounds

A

They are solids in which both cations and anions are present

145
Q

A cation is

A

an atom that has lost electrons

146
Q

What would the charge be on an ion formed from the atom sodium (atomic number 12)

A

+

147
Q

What is the name of the ion with the formula Cr3+

A

Chromium ion

148
Q

A ____ is an atom that has gained one of more electrons and now has a charge

A

Anion

149
Q

A ____ is an atom that has lost one or more electrons and now has a charge

A

Cation

150
Q

What is the charge on the ion formed by the element bromine (atomic number 35)

A

+

151
Q

Ternary acids contains a

A

Halogen

152
Q

H2SO4 is an example of a ____ acid

A

Diprotic

153
Q

What are the ionic compound formulas for

  1. Barium Chloride
  2. Potassium Oxide
  3. Aluminum Phosphide
  4. Magnesium Nitride
A
  1. BaCl2
  2. K2O
  3. AlP
  4. Mg3N2
154
Q

Which of the pairs would most likely form an ionic compound

A) Fe and Ag
B) Ba and O
C) Ca and Ba
D) N and O

A

B) Ba and O

155
Q

Which of the following would most likely form a covalent compound

A) cesium and sodium
B) zinc and sulfur
C) phosphorus and chlorine
D) magnesium and phosphate

A

Phosphorus and chlorine

156
Q

What is the formula for copper (I) oxide

A

Cu2O

157
Q

What are the ionic compounds with their formulas
1. Lithium nitrate
2. Silver sulfate
3. Ammonium sulfide
4. Calcium hydroxide

A
  1. LiNO3
  2. Ag2SO4
  3. (NH4) 2 S
  4. Ca (OH) 2
158
Q

What are the acid names to these formulas

  1. HBr
  2. HNO3
  3. H2SO4
  4. H2CO3
A
  1. Hydrobromic acid
  2. Nitric acid
  3. Sulfuric acid
  4. Carbonic acid
159
Q

Which of these is most likely to form a covalent compound

A) Magnesium and phosphate
B) cesium and sodium
C) sodium and phosphorus
D) sulfur and oxygen

A

Sulfur and oxygen

160
Q

What is the name of the covalent compound with the correct formula

  1. Dinitrogen pentoxide
  2. Phosphorus trichloride
  3. Dichlorine monoxide
  4. Carbon dioxide
A
  1. N2O5
  2. PCl3
  3. Cl2O
  4. CO2
161
Q

Name the covalent compound with its correct formula

  1. Dinitrogen pentoxide
  2. Phosphorus trichloride
  3. Dichlorine monoxide
  4. Carbon dioxide
A
  1. N2O5
  2. PCl3
  3. Cl2O
  4. CO2
162
Q

Name the compound with its correct formula

  1. Iron (III) carbonate
  2. Hydrochloric acid
  3. Sodium sulfate
  4. Sulfur trioxide
  5. Calcium fluoride
A
  1. Fe2(CO3)3
  2. HCl
  3. Na2SO4
  4. SO3
  5. CaF2
163
Q

Name the reaction types
1. 4K + O —> 2 K2O
2. 2KClO3 —> 2KCl + 3 O2
3. 2Al + Fe2O3 —> Al2O3 + 2 Fe
4. 2KNO3 + H2CO3 —> K2CO3 + 2 HNO3
5. 2C8H18 + 25O2 —> 16CO2 + 18H20

A
  1. Synthesis
  2. Decomposition
  3. Single replacement
  4. Double replacement
  5. Combustion
164
Q

What is the normal Ph range of human blood

A

7.35 - 7.45

165
Q

Which of the following is true of Ph

A) It is a measure of the acid and base concentration of a neutral solution

B) It is a measure of the acid concentration of a solution

C) It is a measure of the base concentration of a solution

D) It is a measure of the overall acidity of basicity of a solution

A

It is a measure of the acid concentration of a solution

166
Q

Which of the following is a diprotic acid

A) HCI
B) HNO3
C) H2SO4
D) H3PO4

A

H2SO4

Funeral Service Chemistry (6 decks)

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