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
dL
A. 45,600 dLB. 4.56 dL
C. 0.456 dLD. 0.0456 dLSlide8
Why should excess chemicals never
be
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.
C.
The
excess of chemicals would be shaken when placed back into the original chemical
stock
, thus creating an explosive
environment
.
D.
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?
A.
The
student should immediately begin rinsing his
eyes
at the eye wash station while his partner notifies
the
instructor.
B.
the
student should inform his partner that his eyes are
severely
burned and go to the bathroom for water.
C.
The
student should quickly notify the instructor of
the
problem and ask for permission to rinse his eyes.
D.
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?
A
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?
A
1
. 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
5
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?
A.
2.37%
B.
1.07
%
C.
3.37
%
D.
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
if
the volume is 6.7mL and the mass is 5.67 g.
A.
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
2
2s22p63s2
3p14s2 B. 1s22s22p6
3s
2
3p
3
C. 1s
2
2s
2
2p
6
3s
2
3d
3
D. 1s
2
2s
2
2p
6
3s
2
3p
6
4s
3
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
th
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
B.
ArC. KrD.
Xe
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
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.
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
3
?
A. bentB. trigonal planar
C. tetrahedralD. pyramidal
☺Slide72
What is the shape of BF
3
?
A. trigonal planarB. bent
C. pyramidalD. tetrahedral
☺Slide73
What is the shape of SiO
2
?
A. LinearB. Bent
C. trigonal planarD. pyramidal
☺Slide74
What is the shape of H
2
O?
A. BentB. Linear
C. trigonal planarD. pyramidal
☺Slide75
What is the shape of CH
4
?
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
1+
B. CuC. SD. Ca
2+
☺Slide79
The formula for Lithium Oxide would be
A.
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
3
N2
B. Ca2N3 C. CaND. Ca2
N
2
☺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?
A.
B.
C.D.
☺Slide87
What is the correct electron dot structure for the oxygen ion
A.
B.
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
2
2s
2
2p
6
3s
2
3d
6
C. 1s
2
2s
2
2p
6
3s
2
4p
6
D. 1s
2
2s
2
2p
6
3s
2
3p
5
☺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
2
?
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
2
2s
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
2+
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
2
S?
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
3
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
2
, 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
2
B. KCl
C. POD. NaBr
☺Slide116
Which of the following would contain an ionic bond?
A. HCl
B. MgCl
2
C. N2D. SiH4
☺Slide117
Which structure is nonpolar?
A.
B.
C.
D.
☺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
4
?
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
2
B. Cu
2
Br
2
C. Cu
2
Br
D.
CuBr
☺Slide123
What is the correct name for
(NH
4
)3PO4?
A. Ammonium (I) phosphateB. Ammonium phosphateC.
Ammonium
(
II
) phosphate
D
.
Ammonium
(IV) phosphate
☺Slide124
What is the correct formula for
diphosphorus
pentoxide?
A. P
2
O
2
B. P
5
O
2
C. P
2
O
5
D. PO
5
☺Slide125
What does the roman numeral mean
in
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
3
)
2
A. Calcium dinitrateB. Calcium(II) nitrateC. Calcium nitrateD. Calcium(II) dinitrate
☺Slide127
What is the correct name for MgCO
3
A. Magnesium carbonate
B.
Magnesium(II) carbonateC. Magnesium carbonateD. Magnesium (II) carbonate
☺Slide128
What is the correct name for MnBr
3
?
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
3
P
2?
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
3
B.
Mg2CO3C. Mg(II)CO3 D. Mg3CO
3
☺Slide131
What is the name for Fe(OH)
3
?
A. Iron hydroxide
B. Iron trihyroxideC. Iron (II) hydroxideD. Iron (III) hydroxide
☺Slide132
What is the formula for silver nitrate?
A. Ag
3
NO
3 B. Ag2NO3 C. Ag(I)NO3D.
AgNO
3
☺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)
2?
A. Zinc (I) hydroxideB. Zinc(II) hydroxideC. Zinc(III) hydroxideD. Zinc hydroxide
☺Slide135
What is the name of NH
4
NO
3?
A. Ammonium nitrateB. Nitrogen hydrogen nitrateC. Nitrogen hydroxideD. Ammonium nitride
☺Slide136
The
3 in
NH
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
2
B. MgCl
2C. SO2D. CH4
☺Slide139
Which of the following most likely has an covalent bond?
A.
AlN
B.
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
C.
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
S
A.
hydrosulfuric acidB. dihydrogen sulfideC. hydro(II) sulfuric acidD. sulfurous acid
☺Slide148
Name H2
SO
4
A. Sulfous acid
B. hydrosulfuric acidC. Sulfuric acidD. hydrosulfic acid
☺Slide149
Name HNO2
A.
hydronitriteB. Nitrous acidC. hydronitrite
acidD. hydronitrate
☺Slide150
What is the formula for Nitric acid?
A. HNO
2
B. H2NO3C. H2
NOD. HNO3
☺Slide151
What is the formula for sulfurous acid?
A. H
2
SO3B. H2SO4
C. HSO3D. H2S
☺Slide152
What is the formula for Carbonic acid?
A. H
2
SO3B. H2CO
3 C. H2CO2D. HCO3
☺Slide153
What is the formula for phosphoric acid?
A. H
3
PO4 B. HPO3C. H
3PO2D. HPO2
☺Slide154
What is the formula for hydrochloric acid?
A. H
2
Cl2B. HCl2C. H
2ClD. HCl
☺Slide155
What is the formula for sodium hydroxide?
A. Na
2
(OH)2B. Na(OH)2
C. NaOHD. Na2OH
☺Slide156
What is the formula for Iron(II) hydroxide?
A. Fe(OH)
2
B. Fe2(OH)2C.
FeOHD. Fe(OH)3
☺Slide157
What is the name of Mg(OH)
2
?
A. Magnesium(II) hydroxideB. Magnesium (I) hydroxideC. Magnesic acidD. Magnesium hydroxide
☺Slide158
What is the name of Zn(OH)
2
?
A. Zinc hydroxideB. Zinc(II) hydroxideC. Zinc (I) hydroxideD. Zincic
acid
☺Slide159
What is the name of Mn
(OH)
3
?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
w
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
A
tomic Law
☺