Objective 4

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Objective 4TAKS 10th and 11th grades Home
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Questions from TAKS periodic chart placement
Questions from TAKS balancing equations
Questions from TAKS water properties and
solutions
Questions from TAKS physical and chemical change
Questions from TAKS density
Interactive non-TAKS quizzes on the internet
Link to 10th grade study guide Scroll to p.291
for objective 4
Link to 11th grade study guide Scroll to p.342
for objective 4
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Objective 4 28 questions about chemistry in general Basics and periodic chart An interactive periodic chart A complete tutorial of elements Grades 5 8 quizzes 440 questions...10 per quiz...5 grade levels 20 ques. quiz of basic chem 6 ques. matter 25 ques. chemistry of IPC 8 ques. elements, compounds, mixtures
Objective 4 28 questions about chemistry in general Balance equations Balance equations with instant "right or wrong" Harder balancing equations with instant "right or wrong" 5 question quiz over balancing equations
Objective 4 28 questions about chemistry in general Changes physical or chemical 6 ques. physical/chemical change quiz Powerpoint tutorial physical/chemical changes 8 ques. quiz over physical/chemical changes 10 ques. properties of metals
Objective 4 28 questions about chemistry in general Density, buoyancy, viscosity Density Math --- Click on 'New Problem' ---Have a calculator handy! 10 questions about density reasoning Property of fluids, 8 ques. quiz
Objective 4 28 questions about chemistry in general Water properties 20 difficult water questions. 5 questions Water properties Interactive water molecules/polarity illustrations
Objective 4 28 questions about chemistry in general Solubility 6 ques. Solutions 25 ques. Solubility 12 ques. Solubility factors
Objective 4 28 questions about chemistry in general Electricity and solvents Difficult electronegativity animation Short electrolyte movie
Objective 4 28 questions about chemistry in general pH 25 questions about pH 10 ques. pH and litmus 10 more ques. pH and litmus

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periodic chart placement
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If there are 4 electrons and 4 protons, the
elements atomic number is 4.
The picture shows a model of the element A
fluorine B helium C beryllium D oxygen
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• The elements from which of the following
• groups are most likely to react with
• potassium (K)?
• F Group 2
• G Group 7
• H Group 13
• J Group 17

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1 2 3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
Group 1 wants to give an electron to column
(group) 17
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• An unidentified element has many of the same
  physical and chemical properties as magnesium and
  strontium but has a lower atomic mass than either
  of these elements. What is the most likely
  identity of this element?
• F Sodium
• G Beryllium
• H Calcium
• J Rubidium

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Mass increases with each lower row.
Elements in the same column share the same
physical and chemical properties.
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• The elements of which of these groups on the
  periodic table are most resistant
• to forming compounds?
• A Group 1
• B Group 9
• C Group 14
• D Group 18

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These are the noble gases and they dont like
to bond to anything.
1 2 3 4 5 6 7 8 9 10 11 12
13 14 15 16 17 18
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Elements in Group 16 of the periodic table
usually F form large molecules G gain electrons
when bonding H act like metals J solidify at room
temperature
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These 3 columns gain electrons. They steal
electrons. They need electrons.
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Which of the following groups contains members
with similar chemical reactivity? A Li, Be, C B
Be, Mg, Sr C Sc, Y, Zr D C, N, O
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Elements in the same column have the same
properties and reactivity.
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According to the periodic table, which element
most readily accepts electrons? A Fluorine B
Nitrogen C Arsenic D Aluminum
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Which of the following salts has the greatest
solubility in water at 25C? F CaCO3 G FeS H
HgCl2 J KClO4
Calcium carbonate - insoluble because of rule 3.
Iron sulfide - insoluble because of rule 3
Mercury chloride - insoluble because of rule 2.
Potassium perchlorate - soluble because of rule 1
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An unknown silvery powder has a constant melting
point and does not chemically or physically
separate into other substances. The unknown
substance can be classified as A an element B a
compound C a mixture D an alloy
Compounds can be chemically separated.
Mixtures and alloys can be physically separated.
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Oxygen (O2) is an example of A an alloy B a
molecule C a salt D a mixture
An alloy is a mixture or solution of two metals.
A molecule is two or more atoms bonded covalently
together. Usually included in the bonds are C, P
and the diatomic elements bonded together.
A salt is a an ionic bond between a metal and
non-metal.
A mixture is two substances together but not
bonding together.
A compound can be two or more elements bonded
together, with ionic or metallic bonds.
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balancing equations
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Go to Subscripts
Go to Coefficients
Go to Conservation of mass
Go to Conservation of energy
Balance equations
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Balance equations
According to this information, what is the
chemical formula for aluminum sulfate? A AlSO4 B
Al2(SO4)3 C Al3(SO4)2 D Al6SO4
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The chemical formula for calcium chloride is F
Ca2Cl G CaCl H CaCl2 J Ca2Cl3
Balance equations
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Balance equations
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1 1 1
1 lead 1 lead 2
oxygens ? 3 oxygens
What are the coefficients that will balance this
chemical equation? A 2, 1, 1 B 3, 4, 2 C 2, 2,
1 D 4, 3, 2
Put a 2 here to make an even number of oxygens.
1 lead 2 lead 2
oxygens ? 4 oxygens
2 lead 2 lead 4
oxygens 4 oxygens
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Balance equations
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• When the above equation is balanced, the
• coefficient for magnesium chloride is
• A 0
• B 1
• C 2
• D 4

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Balance equations
2
2
2
1 1
1 1 1
Then well need to put coffecients on this side
of the arrow to finish balancing it out.
To make the hydrogens even, We put the
coefficient 2 here. And have a sum of 4
hydrogens, 2 potassiums and 2 oxygens
What is the coefficient for H2O when the equation
is balanced? A 1 B 2 C 3 D 4
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Balance equations
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Which chemical equation supports the law of
conservation of mass? F 2H2O(l) H2(g)
O2(g) G Zn(s) HCl(aq) ZnCl2(aq)
H2(g) H Al4C3(s) H2O(l) CH4(g)
Al(OH)3(s) J CH4(g) 2O2(g) CO2(g)
2H2O(g)
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Balance equations
4 hydrogens ? 2 hydrogens 2 oxygens 2
oxygens
1 zinc 1 zinc 1 hydrogens ? 2
hydrogens 1 chlorine 2 chlorines
4 aluminums 1 aluminum 3 carbons
1 carbon 2 hydrogens ? 3 hydrogens 1 oxygen
3 oxygens
1 carbons 1 carbon 4 hydrogens 4
hydrogens 4 oxygens 4 oxygens
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To produce 4 molecules of sugar, a plant needs
F 6 molecules of hydrogen G 12 molecules of
ATP H 18 molecules of water J 24 molecules of
carbon dioxide
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Balance equations
Multiply the whole reaction by 4.
4( )
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4 x 6 carbon dioxide
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Balance equations
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100 g
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Balance equations
Reactants ? Products
The chemical equation shows CaCO3 being heated.
Which of these statements best describes the mass
of the products if 100 g of CaCO3 is heated? A
The difference in the products masses is equal
to the mass of the CaCO3. B The sum of the
products masses is less than the mass of the
CaCO3. C The mass of each product is equal to the
mass of the CaCO3. D The sum of the products
masses equals the mass of the CaCO3.
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If all the reactants in a chemical reaction
are completely used, which of the
following statements accurately describes
the relationship between the reactants and
the products? F The products must have a
different physical state than the reactants. G
The total mass of the reactants must equal the
total mass of the products. H The reactants must
contain more complex molecules than the products
do. J The density of the reactants must equal the
density of the products.
Balance equations
Reactants become Products
2H2 O2 ? 2H2O 20 grams 10grams
30 grams
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When 127 g of copper reacts with 32 g of oxygen
gas to form copper (II) oxide, no copper or
oxygen is left over. How much copper (II) oxide
is produced? F 32 g G 95 g H 127 g J 159 g
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Balance equations
127 32 ?
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Balance equations
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Balance equations
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According to the law of conservation of mass, how
much zinc was present in the zinc carbonate? A 40
g B 88 g C 104 g D 256 g
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Balance equations
64 192 152 ? 64 192 152 ?
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Balance equations
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Balance equations
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The energy not stored in the bonds of the carbon
dioxide and water must have left in the form of
heat.
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Balance equations
?


Reactants Products
Why is the sum of the products energy in this
reaction less than the sum of the reactants
energy? A Energy is given off as heat. B The
products absorb available energy. C Energy is
trapped in the reactants. D The reactants energy
is less than the melting point of glucose.
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After
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Balance equations
The illustrations show a conservation-of-mass expe
riment. The solution in the beaker lost mass
because F materials have less mass at high
temperatures G the mass of the reactants and
products was less than 100 g H sodium sulfate
(Na2SO4) is lighter than air J some of the water
molecules turned into gas
Before
Some of the water evaporated because of the heat.
Before(100 g)
After( less than 100 g)
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REACTANTS ?Products The sum of the reactants
the sum of the products.
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An inventor claims to have created an internal
combustion engine that converts 100 kJ of
chemical energy from diesel fuel to 140 kJ of
mechanical energy. This claim violates the law of
conservation of F momentum G inertia H
energy J mass
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Balance equations
chemical energy mechanical energy heat
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water properties
Back to water
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Go to Polarity
Go to Solubility of liquids, solid
Go to Solubility of gases in liquids
Go to Electrolytic behaviors of solutions
Go to pH
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Back to water
What characteristic of water remains the same no
matter what is dissolved in it? A The ratio of
hydrogen to oxygen B The ability to refract
light C The hydroxide ion concentration D The
freezing temperature
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Water is defined as two hydrogens to one oxygen.
If there were more or less of these elements, the
compound would have a different name and not be
water.
The bending of light depends on temperature and
whether there is any solute in the water.
Usually, the amount of OH- and H ions are equal
in pure water.
Water that is not pure, such as with solutes,
does not always freeze at 0oC.
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Which factor makes water an effective solvent? F
The presence of molecular oxygen G Its lack of
covalent bonds H The polar nature of its
molecules J Its abundance on Earths surface
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What is polarity?
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• polarity a compounds uneven distribution of
  electrons.

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Polarity acts like magnets.

• polarity a compounds uneven distribution of
  electrons.

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The hydrogens are attracted to the oxygens of
another molecule.

• polarity a compounds uneven distribution of
  electrons.

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What does polarity do?
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Causes water to expand when it freezes.
ice
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Fish survive through severe winters because of
the property of water that allows water to F
form chemical bonds as it freezes, raising the
water temperature below the ice G increase in
density while it freezes, dissolving more oxygen
from the air H expand when it freezes, creating a
floating and insulating layer of ice J
precipitate vital nutrients when it freezes,
increasing the food supply
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Freezing water becomes less dense.
The air above the ice may be very, very cold

even - 60oF. But the water beneath
the ice is no colder than 33oF. The living
things in the very cold water have adaptations
for 33oF but may not be able to survive any
colder water than that.
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If the properties of water were to change so that
the solid form was denser than the liquid form,
organisms living in a cold pond environment would
be less likely to survive because water would no
longer F dissolve enough oxygen from the air G
produce solutions containing vital
nutrients H remain neutral, instead becoming
highly acidic J produce a floating
insulating layer of ice
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Back to water
Salt ions being separated by collisions of water
molecules during dissolving.
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What are some solubility tricks?
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• Grind large pieces of solute into small pieces,
  thereby increasing surface area for the water
  molecules to collide into.
• Raise the temperature to increase collisions of
  H2Os into solute.
• Stir or shake which increases the collisions.

surface area smaller particles have more
surface area compared to one large particle.
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surface area smaller particles have more
surface area compared to one large particle.
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A 0.2 g crystal of gypsum dissolves very slowly
in 100 mL of water while the water is stirred.
Which of these would cause the gypsum to dissolve
faster? F Decreasing the water temperature G
Stopping the stirring H Lowering the air
pressure J Crushing the crystal
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All of these can affect the rate at which a solid
dissolves in water except A decreasing air
pressure B stirring the water C increasing the
temperature of the water D using larger crystals
of the solid
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Air pressure only affects gas solubility.
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As a scuba diver goes deeper underwater,
the diver must be aware that the
increased pressure affects the human body by
increasing the A bodys temperature B amount of
dissolved gases in the body C amount of suspended
solids in the body D concentration of minerals in
the body
Going deeper under water, the gasses of the
blood become more condensed and dissolved.
Coming up too fast, is like shaking a can of
coke and then opening up. The body doesnt like
it. Its called the bends.
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Over time an open soft drink will lose
carbonation (dissolved CO2). Which of these
allows the CO2 to remain in solution the
longest? A Reduced air pressure B Exposure to
direct sunlight C Increased air currents D Cooler
temperatures
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Carbon dioxide Gas
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Which bottle will lose its dissolved carbon
dioxide to the atmosphere soonest?
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How does temperature affect solubility?
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How does pressure affect solubility?The more
pressure (lid on) the better the dissolving of a
gas in a liquid.
But gases dissolve better at lower temperatures.
Usually, the warmer, the better.

• The table shows temperature and pressure in four
  containers holding the same amount of water.
  According to the table, in which container can
  the most sodium chloride be dissolved in the
  water?
• A Q
• B R
• C S
• D T

Rule With solubility of most salts, temperature
is more important than pressure.
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The word BRIGHT Means the liquid is A strong
electrolyte.

• In this apparatus, the seawater is an example of
  a
• F strong electrolyte
• G weak acid
• H nonelectrolyte
• J strong base

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Salt ions being separated by collisions of water
molecules during dissolving.
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Bathwater normally has electrolytic behaviors
even though distilled water does not. This is
because bathwater F contains isotopes of
hydrogen G has been heated H is separated into H
and OH ions J contains dissolved minerals
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Isotopes are elements with different number of
neutrons although they have the same number of
electrons and protons.
Heating water does NOT make the water an
electricity carrier. Ions in the water, make
water carry electricity.
Elements of water are covalently bonded meaning
that they resist becoming ions. Some always do,
but they do not conduct electricity because they
are so attracted to the opposite ion.
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Sour Slippery
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pH indicators
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pH paper tells pH numbers
Litmus paper tells acid or base
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A certain commercial product used for cleaning
ovens must be handled with rubber gloves. The
product is slippery and turns litmus paper blue.
It probably contains F an acid G a base H a
salt J an isotope
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Back to water
Two clear solutions are placed in separate
beakers. The first solution has a pH of 4, and
the pH of the second solution is unknown. If the
two solutions are mixed and the resulting pH is
5, the second solution must have A fewer
suspended solids B a lower temperature C more
dissolved salt (NaCl) particles D a higher
concentration of OH ions
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Acid pH 4
Base with some OHs
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Acid Base becomes Salt Water
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• Many pitcher-plant species grow well in soil with
  a low pH. Soil pH could be decreased by adding a
  solution of
• A carbonic acid
• B potassium hydroxide
• C ammonia
• D sodium chloride

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physical and chemical change
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• Which of the following processes is an
• example of a physical change associated with
• an oak tree?
• A Decomposition of bark by bracket fungi
• B Starches and sugars being broken down during
  energy production
• C Water and carbon dioxide being converted to
  glucose
• D Evaporation of water from the surfaces of leaves

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Chemical change
Chemical change
Chemical change
Physical change
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Chemical changes Bonding partners are changed.
Milk sugar proteins ? carbon dioxide water
other chemicals
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Which of the following is an example of a
chemical change? F Ice cracking G Sugar
dissolving H Milk souring J Lead melting
Physical changes Getting smaller Dissolving Chang
ing phasessolid,liquid,gas
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• Which of these changes in rocks is a physical
  change?
• A Acid rain damaging marble
• B Iron in rock combining with oxygen to
• form hematite
• C Carbonic acid weathering limestone
• D An ice wedge shattering a slab of shale

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Which process in the rock cycle is most likely
responsible for moon rocks being converted to
lunar soil? A Metamorphism B Weathering C
Sedimentation D Volcanism
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Reheating of rocks.
Weathering changes rock to soil on the earth, so
it might apply to the moon as well.
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Which of these describes a pollution-producing pro
cess that involves only a physical change? A
Coal with a high sulfur content is
burned, producing gases that cause acid rain. B
Chlorofluorocarbons are released, changing ozone
in the upper atmosphere into oxygen. C Hot
wastewater is discharged into a lake, lowering
oxygen levels in the water. D Nitrogen oxide
emissions combine with water vapor, producing
nitric acid.
Normal environment
Coal S Oxygen ? CO2 SO3 H2O ?
H2SO4
Hot water is added to a river
or lake.
Warmed Oxygen O2 bubbles to atmosphere.
O3 ? O2 O1 with the
Thermal pollution causes a physical change.
NO2 H2O ? HNO3
Decrease in dissolved oxygen causes fish kill.
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In the rock cycle, which of these is a chemical
change involved with the formation of igneous
rocks? F Compression of sediments G Heat loss
from lava H Subduction of plates J Formation of
minerals
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May cause a chemical change with pressure.
May result from chemical changes.
Is the act of elements unbonding and rebonding.
May cause a chemical change with heat/friction.
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density
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A block of maple wood with a volume of 405 cubic
centimeters and a density of 0.67 g/cm3 is sawed
in half. The density of the two smaller blocks is
now A one-fourth the original density B
one-half the original density C two times the
original density D the same as the original
density
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If all these blocks are maple, they all have the
same density.
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A sample of an element has a volume of 78.0 mL
and a density of 1.85 g/mL. What is the mass in
grams of the sample? Record and bubble in your
answer to the nearest tenth on the answer
document.
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Density mass volume 1.85 ? 78 1.85 x 78
?
144.3 grams
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Which procedure is best to use when determining
the density of a rock? F Place the rock in a
water-filled beaker and find the height at which
the rock floats above the water. G Use a ruler to
measure the rocks dimensions and then find its
mass using an analytical balance. H Measure the
mass of the rock on a balance and then find the
volume of water it displaces in a graduated
cylinder. J Place the rock in three liquids with
different known densities and observe which
liquid the rock floats in.
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161.02 22.35 139.67
Density mass / volume Density 139.67g / 20.1
mL
60.4 40.3 20.1
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Which of the following objects will float on
water?
55/50 greater than 1
45/40 greater than 1
Density greater than 1 sinks. Density less than
1 floats.
50/45 greater than 1
60/65 less than 1
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What is the mass of a 500.00 mL sample
of seawater with a density of 1.025 g/mL? F 487.8
g G 500.0 g H 512.5 g J 625.0 g
Density mass volume 1.025 ? 500 500 x
1.025 ?
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Gases have a greater volume than liquids.

• Compared to 250 g of gaseous nitrogen, 250 g of
  liquid nitrogen has greater
• A volume
• B temperature
• C mass
• D density

Density is mass / volume
Gas N2 Liquid N2
250/big number 250/small number
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Density less than 1 floats on water. Density
more than 1 sinks in water.

• 17 Swimmers find that they can float more easily
  in the ocean than in a freshwater pond. The most
  likely reason for this phenomenon is that the
• A viscosity of pond water is greater than that of
  ocean water
• B density of ocean water is higher than that of
  pond water
• C temperature of pond water is lower than that of
  ocean water
• D mass of ocean water is greater than that of
  pond water.

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From 1942 to 1945, U.S. nickels were made of an
alloy that contained 35 silver, 9.0 manganese,
and the rest copper, by mass. If one of these
nickels has a mass of 5.0 grams, what is the mass
of the copper? A 0.5 g B 1.8 g C 2.2 g D 2.8 g
Silver manganese copper 100
Copper 100 - 35- 9
Copper 56 or
56/100 or .56 56 / 100 x 5
grams 2.8 grams or .56 x 5 2.8
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What is the density at 20C of 12.0 milliliters
of a liquid that has a mass of 4.05 grams? A
0.338 g/mL B 2.96 g/mL C 16.1 g/mL D 48.6 g/mL
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Dont need temp.
Density mass volume ? 4.05 g
12mL
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This pipette is filled with a 20 NaOH solution.
The solution is at 20C and has a density of 1.23
g/mL. According to this information, what is the
mass of this NaOH solution? A 3.88 g B 15.7 g C
23.9 g D 24.6 g
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D m V D x V m 1.23 x amount in graduated
cylinder mass
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