Exam Review 2019 Ch. 1-9 - PowerPoint Presentation

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Exam Review 2019 Ch. 1-9 - PPT Presentation

What is the following and what is it used for A test tube holder holding test tubes B double buret clamp holding burets C forceps picking up small objects D crucible tongs holding crucibles ID: 758364

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Slide1

Exam Review

2019 Ch. 1-9Slide2

What is the following and what is it used for?

A. test tube holder, holding test tubes

B. double buret clamp, holding burets

C. forceps, picking up small objectsD. crucible tongs, holding cruciblesSlide3

Which of these would be best to measure 14.2 mL of liquid water?

A 25 mL volumetric flask

B 25 mL graduated cylinder

C 25 mL Erlenmeyer flask D 25 mL beakerSlide4

The figure shows an experimental setup used to separate the components of a colored ink sample. Which of the following describes this laboratory technique?

A Filtration

B Decanting

C Chromatography

D DistillationSlide5

The volume of the hammer is approximately—

A 5 mL

B 64 mL

C 4 mL D 69 mLSlide6

What is the following and what is it used for?

A. test tube holder, holding test tubes

B. double buret clamp, holding burets

C. forceps, picking up small objectsD. crucible tongs, holding cruciblesSlide7

Convert 456 m

L to

A. 45,600 dLB. 4.56 dL

C. 0.456 dLD. 0.0456 dLSlide8

Why should excess chemicals never

returned to reagent bottles?

A.The entire stock bottle of the chemical would be contaminated if the container holding the

excess chemicals has some contamination.B.A spill could be created if excess chemicals are poured from the retaining bottle to the

original

chemical stock bottle.

The

excess of chemicals would be shaken when placed back into the original chemical

stock

, thus creating an explosive

environment

The

excess chemical would spoil because it was exposed to

additional

oxygen when placed in a retaining bottle.Slide9

What is the following and what is it used for?

A. crucible, heating to high temperatures

B. graduated cylinder, measuring volume

C. watch glass, covering evaporating dishD. evaporating dish, evaporatingSlide10

A student did not follow proper safety

procedures

while conducting a chemistry experiment and forgot to

wear safety goggles. During the experiment an acidic solution splashed into the student's eyes causing

severe pain. What are the correct steps that the student should have taken during this emergency?

The

student should immediately begin rinsing his

eyes

at the eye wash station while his partner notifies

the

instructor.

the

student should inform his partner that his eyes are

severely

burned and go to the bathroom for water.

The

student should quickly notify the instructor of

the

problem and ask for permission to rinse his eyes.

The

student should ask the instructor for permission to

visit

the school nurse. Slide11

What is the following and what is it used for?

A. crucible, heating to high temperatures

B. graduated cylinder, measuring volume

C. watch glass, covering evaporating dishD. evaporating dish, evaporatingSlide12

If a student's hand is accidentally exposed to an acidic solution, what should be done?

Rinse

the hand in cold running water B Wrap the hand in paper towels

C Cover the hand with oil D Rinse the hand in a concentrated baseSlide13

What is the following and what is it used for?

A. test tube holder, holding test tubes

B. double buret clamp, holding burets

C. forceps, picking up small objectsD. crucible tongs, holding cruciblesSlide14

What is the correct order to add water and acid together?

. Acid is poured into a beaker. 2. Water and salt are then poured into the beaker with acid. B1. Acid is poured into a beaker. 2. Water is then poured into the beaker with acid.

C1. Water is poured into a beaker. 2. Acid is then poured into the beaker with water. D1. Water and salt are poured into a beaker. 2. Acid is then poured into the beaker with water.Slide15

If you dissolve sugar in different types of solvents to determine which solvent dissolves the sugar fastest, what is the independent variable.

A. amount of sugar

B. amount of solvent

C. time to dissolve

D. type of solventSlide16

If you dissolve sugar in different types of solvents to determine which solvent dissolves the sugar fastest, what is the dependent variable.

A. amount of sugar

B. amount of solvent

C. time to dissolve

D. type of solventSlide17

Why do experiments do many trials?

A. So the results can be averaged to give a more accurate result.

B. So the results can be published in multiple data tables.

C. So that each lab group has a chance to do the experimentD. So that more material can be used up during experimentationSlide18

What is the following and what is it used for?

A. crucible, heating to high temperatures

B. graduated cylinder, measuring volume

C. watch glass, covering evaporating dishD. evaporating dish, evaporatingSlide19

What is the following and what is it used for?

A. test tube holder, holding test tubes

B. double buret clamp, holding burets

C. forceps, picking up small objects

D. crucible tongs, holding cruciblesSlide20

What is the correct reading for significant figures?

A. 146.44

B. 146.4

C. 146.440

D. 146Slide21

What is the following and what is it used for?

A. crucible, heating to high temperatures

B. graduated cylinder, measuring volume

C. watch glass, covering evaporating dishD. evaporating dish, evaporatingSlide22

4.2089300 X 10

g expresses how many significant figures?

A. 5B. 6C. 8D. 9Slide23

A student measured the density of an

object three

times. He recorded the following density measurements:

1.50 g/mL, 1.60 g/mL, and

1.30 g/mL. The actual density of this object is 1.49 g/mL.

After finding the average of the

student's

measurements, what was

the

percent error between the student's average

measurement

of density and the actual density of the object?

2.37%

1.07

3.37

1.34

%Slide24

Which of the following contains the greatest number of significant digits?

A. 45.0 g

B. 60.090 g

C. 606000 gD. 7.040 gSlide25

Add the following and choose the answer with the correct number of significant digits.

4.5 g + 9.08 g + 8.98 g=?

A. 22 g

B. 22.56 g

C. 22.5 gD. 22.6 gSlide26

When the products of a reaction have different chemical properties than the reactants that formed them, it is an indication that

A. a chemical change has occurred

B. no change has occurred

C. the reactants are contaminated

C. a physical change has occurredSlide27

A chemical property would include

A. boiling point

B. crystalline structure

C. freezing pointD. decompositionSlide28

What is this a picture of?

A. heterogeneous mixture

B. homogeneous mixture

C. colloidD. sublimationSlide29

Calculate the density with the correct number of significant figures

the volume is 6.7mL and the mass is 5.67 g.

1.2 g/mLB. 0.8463 g/mLC. 0.85 g/mLD. 0.846 g/mLSlide30

How does ionization energy trend within a period?

A. it increases

B. it decreases

C. it plateausD. it stays constant

Slide31

Which element has the smallest atomic radius?

A. Mg

B. P

C. CaD. Cl

Slide32

How does shielding trend across a period?

A. it increases

B. it decreases

C. it plateausD. it stays constant

Slide33

What is the electron configuration of Phosphorus?

A. 1s

2s22p63s2

3p14s2 B. 1s22s22p6

C. 1s

D. 1s

Slide34

Which block are the alkali metals in?

A. s block

B. p block

C. d blockD. f block

Slide35

Which block are the transition metals in?

A. s block

B. p block

C. d blockD. f block

Slide36

Which block are the inner transition metals in?

A. s block

B. p block

C. d blockD. f block

Slide37

Which block are the noble gases in?

A. s block

B. p block

C. d blockD. f block

Slide38

The atomic number is

always

equal to the number of

A. electronsB. neutronsC. protons and electronsD. protons

Slide39

Nitrogen- 16 has ___ neutrons and ___ protons

A. 9,7

B. 7,9

C. 16,7D. 7,16

Slide40

A neutral atom of an element has the same number of ____ as protons.

A. neutrons

B. electrons

C. neutrons and electronsD. particles

Slide41

Dalton speculated that atoms of the same element are _____________ to one another.

A. identical

B. larger

C. smallerD. different



He was wrong!Slide42

Isotopes of an element differ in the number of

A. electrons

B. protons

C. neutronsD. alpha particles

Slide43

Calculate the average atomic mass of a sample that is 80% Fe-55 and 20% Fe-56.

A. 55.5

B. 55.8

C. 55.2D. 55.0

Slide44

What particle has a negative charge and is 1/2000

the mass of a proton?

A. neutronB. protonC. electronD. alpha particle

Slide45

How does electronegativity trend down a group?

A. it increases

B. it decreases

C. it plateausD. it stays constant

Slide46

How does electronegativity trend across a period?

A. it increases

B. it decreases

C. it plateausD. it stays constant

Slide47

What did J.J. Thompson discover that were later called electrons?

A. positive particles he called corpuscles

B. negative particles he called corpuscles

C. neutral particles he called corpusclesD. negative particles he called neutrons

Slide48

Groups 1A-7A are called

A. transition elements

B. representative elements

C. alkali metalsD. noble gases

Slide49

Group 3-12 are called

A. transition elements

B. representative elements

C. alkali metalsD. noble gases

Slide50

Groups 3A-7A have incomplete __ sublevels.

A. s

B. p

C. dD. f

Slide51

Transition metals have incomplete __ sublevels

A. s

B. p

C. dD. f

Slide52

Horizontal rows are called ___ and vertical columns are called ___ on the periodic table.

A. periods, groups

B. groups, periods

C. transition, representativeD. representative, transition

Slide53

Noble gases are ___ because they have ___ outer energy levels.

A. reactive, filled

B. inert, partially filled

C. inert, filledD. reactive, partially filled

Slide54

Which of these has the highest electronegativity?

A. Be

B. N

C. NeD. Li

Slide55

Which of the following has the highest electronegativity?

A. O

B. S

C. CsD. Fr

Slide56

Noble gases are in group

A. 1A

B. 7A

C. 2AD. 8A

Slide57

5th

Slide58

Alkaline Earth Metals are in group

A. 1A

B. 7A

C. 2AD. 6A

Slide59

Convert 456 dL

to mL

A. 456,000 mL

B. 45,600 mLC. 0.456 mLD. 0.0456 mLSlide60

Alkali metals are in group

A. 1A

B. 7A

C. 3AD. 6A

Slide61

80% of the periodic table is

A. non-metals

B. transition elements

C. metalsD. solid

Slide62

In general, ___ are on the left side of the metalloid “stair-step” and ___ are on the right side of the metalloid “stair-step”.

A. metals, nonmetals

B. metalloids, gases

C. gases, solidsD. p orbitals, s orbitals

Slide63

Which noble gas would be used to write a noble gas configuration for magnesium?

A. Ne

ArC. KrD.

Slide64

Elements in the same group have the same number of

A. neutrons in highest occupied energy level

B. protons in the highest occupied energy level

C. alpha particles in the highest occupied energy levelD. electrons in the highest occupied energy level

Slide65

What is Hund’s

Rule?

A. All electrons are negative

B. One electron occupies each orbital in a sublevel before a second one is added.C. Only two electrons are allowed in each orbital and they must have opposite spins.D. Electrons fill lower energy levels before filling higher energy levels.

Slide66

What is the Pauli Exclusion Principle?

A. All electrons are negative

B. One electron occupies each orbital in a sublevel before a second one is added.

C. Only two electrons are allowed in each orbital and they must have opposite spins.

D. Electrons fill lower energy levels before filling higher energy levels.

Slide67

What is the Aufbau

Principle?

A. All electrons are negative

Slide68

Make sure you know orbital notation and can recognize if

Hund’s

Rule, Pauli Exclusion Principle or the

Aufbau Principle is not followed!!Slide69

Cations are formed when neutral

A. atoms lose electrons

B. atoms gain electrons

C. atoms gain protonsD. atoms lose neutrons

☺Slide70

The formula for magnesium oxide is

A. MgO

B. Mg

2OC. MgO

2D. Mg2O2

☺Slide71

What is the shape of NH

A. bentB. trigonal planar

C. tetrahedralD. pyramidal

☺Slide72

What is the shape of BF

A. trigonal planarB. bent

C. pyramidalD. tetrahedral

☺Slide73

What is the shape of SiO

A. LinearB. Bent

C. trigonal planarD. pyramidal

☺Slide74

What is the shape of H

A. BentB. Linear

C. trigonal planarD. pyramidal

☺Slide75

What is the shape of CH

A. pyramidalB. tetrahedral

C. trigonal planarD. bent

☺Slide76

Valence electrons are found in the _____ energy level of an atom.

A. innermost

B. weakest

C. outermostD. lowest

☺Slide77

Which element has one less valence electron than Carbon?

A. Be

B. N

C. SiD. B

☺Slide78

Which atom or ion has the electron configuration of a noble gas?

A. Mg

B. CuC. SD. Ca

☺Slide79

The formula for Lithium Oxide would be

LiO

B. LiO2

C. Li2O2 D. Li2O

☺Slide80

Which element has three valence electrons?

A. Al

B. Si

C. GeD. S

☺Slide81

Which element would be used to write the noble gas configuration of Aluminum?

A. He

B. Ne

C. Kr

D. Ar

☺Slide82

What type of bonds are in ethanol?

A. ionic

B. nuclear

C. metallic

D. covalent

☺Slide83

Which of the following would be polar?

A. He

B. N

2C. SiO

2D. SeO2

☺Slide84

The correct formula for Calcium Nitride would be

A. Ca

B. Ca2N3 C. CaND. Ca2

☺Slide85

Electrons are __, neutrons are __ and protons are __

A. positive, negative, neutral

B. negative, positive, neutral

C. positive, neutral, negativeD. negative, neutral, positive

☺Slide86

Which is the correct electron dot structure for Nitrogen?

C.D.

☺Slide87

What is the correct electron dot structure for the oxygen ion

C.D.

☺Slide88

What is modeled as a sea of electrons?

A. valence electrons in non metals

B. valence electrons in gases

C. valence electrons in solidsD. valence electrons in metals

☺Slide89

What is the electron configuration of Cl

A. 1s2

2s22p63s23p6 B. 1s

C. 1s

D. 1s

☺Slide90

An oxygen ion has the same number of electrons as a neutral atom of

A. He

B. Ne

C. Ar

D. Kr

☺Slide91

A(n) ______ has superior properties to the metals they are composed of.

A. alkali metal

B. alloy

C. alkaline earth metal

D. noble gas

☺Slide92

The ______of an ion is equal to the sum of the positive charge of each proton and the negative charge of each electron.

A. mass

B. energy

C. charge

D. electronegativity

☺Slide93

_______ are formed when neutral atoms gain electrons.

A. anions

B. cations

C. atomsD. metals

☺Slide94

Ionic compounds when dissolved in water ___

A. melt

B. conduct electricity

C. heat upD. cool down

☺Slide95

How many electrons does the copper ion have when it forms the ionic compound CuCl

A. 29

B. 28C. 27D. 26

☺Slide96

What kind of bond involves the transfer of electrons?

A. covalent

B. ionic

C. complexD. metallic

☺Slide97

An atom with an electron configuration of 1s

22p63s23p

2 is most likely to form an ion that has a charge of

A. 2

B. 4

C. 3

D. 2

☺Slide98

The Ca

ion contains __ electrons.

A. 20B. 19 C. 18

D. 17

☺Slide99

An ion that has 9 protons and 10 electrons is

A. Ne

B. F+

C. Ne-D. F-

☺Slide100

Cations are __ and Anions are ___

A. negative, positive

B. positive, negative

C. neutral, negativeD.

positive,neutral

☺Slide101

Representative elements lose or gain electrons to gain the ___ of a noble gas.

A. electronegativity

B. ionization energy

C. atomic radius

D. electron configuration

☺Slide102

__ play a necessary function in chemical reactions called bonding.

A. protons

B. electrons

C. neutronsD. alpha particles

☺Slide103

Transferring of electrons between atoms would describe a(n)

A. splitting bond

B. ionic bond

C. covalent bond

D. molecular bond

☺Slide104

When a metal and a nonmetal form a bond you would expect what type of bond?

A. ionic

B. covalent

C. metallic

D. molecular

☺Slide105

When two nonmetals form a bond, you would expect

A. transfer of electrons for a covalent bond

B. sharing of electrons for an ionic bond

C. sharing of electrons for a covalent bond

D. transfer of electrons for an ionic bond

☺Slide106

Electrons can be lost, shared or ____ during bonding processes.

A. gained

B. demoted

C. emitted

D. spun off

☺Slide107

Which element will form a covalent bond with oxygen?

A. neon

B. phosphorus

C. potassium

D. magnesium

☺Slide108

When nitrogen triple bonds with another nitrogen atom, there are

A. no lone pairs of electrons on either nitrogen atom

B. two lone pairs of electrons on each nitrogen atom

C. one lone pair of electrons on each nitrogen atom

D. one lone pair of electrons on only one of the nitrogen atoms

☺Slide109

What types of bonds can be found in a solid sample of H

A. covalent bonding only

B. both ionic and covalent bondingC. hydrogen bonding onlyD. both covalent and hydrogen bonding

☺Slide110

Which of the following would be nonpolar?

A BF

B. H

2SeC. SiH4D. H2Se

☺Slide111

Which element does not naturally occur as a diatomic molecule?

A. H

B. Br

C. N

D. C

☺Slide112

The

lewis

dot structure for a molecule of C

2H4 would have

A. five single bondsB. four single bonds and one double bondC. 3 single bonds and two double bondsD. 2 single bonds and 2 double bonds

☺Slide113

What type of bond forms in N

, Br

2 and O2

A. an ionic bond formed by the gain of electronsB. a covalent bond formed by the sharing of electronsC. a metallic bond formed by the transfer of electronsD. a nuclear bond formed by the sharing of electrons

☺Slide114

If all of the electrons are distributed ____ in a molecule, the molecule is non-polar.

A. equally

B. within p orbitals

C. unequally

D. randomly

☺Slide115

Which compound would have a covalent bond?

A. CaBr

B. KCl

C. POD. NaBr

☺Slide116

Which of the following would contain an ionic bond?

A. HCl

B. MgCl

C. N2D. SiH4

☺Slide117

Which structure is nonpolar?

☺Slide118

This shows the formation of a _____ bond.

A. non polar covalent

B. polar covalent

C. metallic

D. non polar ionic

☺Slide119

How many bonds are shown in the structural formula below?

A. 1 covalent, 8 ionic

B. one double covalent, 8 ionic

C. 8 double covalent, 1 single covalent

D. 1 double covalent, 8 single covalent

☺Slide120

When a molecule is polar, it behaves as if one end of the molecule is ___ and the other end of the molecule is ___.

A. negative, positive

B. magnetic, nonmagnetic

C. ionic, nonionic

D. neutral, positive

☺Slide121

What is the correct name for CrSO

A. Chromium (I) sulfateB. Chromium (II) sulfate

C. Chromium (III) sulfateD. Chromium (IV) sulfate

☺Slide122

What is the correct formula for copper(II)bromide?

A. CuBr

B. Cu

C. Cu

CuBr

☺Slide123

What is the correct name for

(NH

)3PO4?

A. Ammonium (I) phosphateB. Ammonium phosphateC.

Ammonium

(

) phosphate

Ammonium

(IV) phosphate

☺Slide124

What is the correct formula for

diphosphorus

pentoxide?

A. P

B. P

C. P

D. PO

☺Slide125

What does the roman numeral mean

copper(II)bromide?

A. number of molecules

B. number of atomsC. number of valence electronsD. charge on the ion

☺

☺Slide126

What is the correct name for Ca(NO

)

A. Calcium dinitrateB. Calcium(II) nitrateC. Calcium nitrateD. Calcium(II) dinitrate

☺Slide127

What is the correct name for MgCO

A. Magnesium carbonate

Magnesium(II) carbonateC. Magnesium carbonateD. Magnesium (II) carbonate

☺Slide128

What is the correct name for MnBr

A. Manganese(I) bromide(III)

B. Manganese(III) bromide(III)C. Manganese bromide (III)D. Manganese(III) bromide

☺Slide129

What is the? correct name for Fe

A. Iron (III) phosphideB. Iron (II) phosphideC. Iron phosphideD. Iron (II) phosphide(III)

☺Slide130

What is the correct formula containing magnesium and carbonate?

A. MgCO

Mg2CO3C. Mg(II)CO3 D. Mg3CO

☺Slide131

What is the name for Fe(OH)

A. Iron hydroxide

B. Iron trihyroxideC. Iron (II) hydroxideD. Iron (III) hydroxide

☺Slide132

What is the formula for silver nitrate?

A. Ag

3 B. Ag2NO3 C. Ag(I)NO3D.

AgNO

☺Slide133

What is

the name of

Cd(CO

3)2?

A. Cadmium(I) carbonateB. Cadmium(II) carbonateC. Cadmium(III) carbonateD. Cadmium carbonate

☺Slide134

What is

the name of

Zn(OH)

A. Zinc (I) hydroxideB. Zinc(II) hydroxideC. Zinc(III) hydroxideD. Zinc hydroxide

☺Slide135

What is the name of NH

A. Ammonium nitrateB. Nitrogen hydrogen nitrateC. Nitrogen hydroxideD. Ammonium nitride

☺Slide136

The

3 in

4NO3is a(n)

A. coefficientB. subscriptC. oxidation numberD. exponent

☺Slide137

What element has the same

electron dot structure as boron?

Carbon

Nitrogen

Oxygen

Aluminum

☺Slide138

Which of the following most likely has an ionic bond?

A. H

B. MgCl

2C. SO2D. CH4

☺Slide139

Which of the following most likely has an covalent bond?

AlN

KClC. CaOD. CO

☺Slide140

When ionic compounds are named, the name of the anion (if it’s not polyatomic!) will be

A. –

ite

B. –ide

C. –icD. -ate

☺Slide141

Which particles are lost, shared or gained when bonding?

A. protons

B. electrons

C. neutrons

D. alpha particles

☺Slide142

In most cases, how many valence electrons are needed for stability?

A. 2

B. 4

C. 6

D. 8

☺Slide143

Which noble gas has an electron configuration that is stable with only two electrons?

A. H

B. He

ArD. Kr

☺Slide144

When hydrogen bonds covalently with fluorine, hydrogen shares ___ pair(s) of electrons.

A. 1

B. 2

C. 3

D. 4

☺Slide145

Ionic bonds occur between cations and ___

A. hydrogen ions

B. anions

C. polar molecules

D. coordinate covalent bonds

☺Slide146

Name HF

A. hydrogen fluoride

B. hydrogen

trifluorideC. hydric acidD. hydrofluoric acid

☺Slide147

Name H2

hydrosulfuric acidB. dihydrogen sulfideC. hydro(II) sulfuric acidD. sulfurous acid

☺Slide148

Name H2

A. Sulfous acid

B. hydrosulfuric acidC. Sulfuric acidD. hydrosulfic acid

☺Slide149

Name HNO2

hydronitriteB. Nitrous acidC. hydronitrite

acidD. hydronitrate

☺Slide150

What is the formula for Nitric acid?

A. HNO

B. H2NO3C. H2

NOD. HNO3

☺Slide151

What is the formula for sulfurous acid?

A. H

SO3B. H2SO4

C. HSO3D. H2S

☺Slide152

What is the formula for Carbonic acid?

A. H

SO3B. H2CO

3 C. H2CO2D. HCO3

☺Slide153

What is the formula for phosphoric acid?

A. H

PO4 B. HPO3C. H

3PO2D. HPO2

☺Slide154

What is the formula for hydrochloric acid?

A. H

Cl2B. HCl2C. H

2ClD. HCl

☺Slide155

What is the formula for sodium hydroxide?

A. Na

(OH)2B. Na(OH)2

C. NaOHD. Na2OH

☺Slide156

What is the formula for Iron(II) hydroxide?

A. Fe(OH)

B. Fe2(OH)2C.

FeOHD. Fe(OH)3

☺Slide157

What is the name of Mg(OH)

A. Magnesium(II) hydroxideB. Magnesium (I) hydroxideC. Magnesic acidD. Magnesium hydroxide

☺Slide158

What is the name of Zn(OH)

A. Zinc hydroxideB. Zinc(II) hydroxideC. Zinc (I) hydroxideD. Zincic

acid

☺Slide159

What is the name of Mn

(OH)

?A. Manganese hydroxide B. Manganese (I) hydroxideC. Manganese(III) hydroxide

D. Manganic acid

☺Slide160

Which law

states that in samples of any chemical compound, the masses of the elements are always in the same proportions.

A. Law of multiple proportions

B. Law of definite proportions

C. Law of conservation of energyD. Law of entropy

☺Slide161

Which law states

henever

the same two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers.

A. The Law of Multiple Proportions

B. The Law of Definite Proportions

C. The Law of Conservation of Matter

D. Dalton’s

tomic Law

☺