Download - TAKS Review Ppt Objective 4
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Structure & Structure & Properties of Properties of
MatterMatter
Science TAKSScience TAKS ReviewReview
Objective 4Objective 4
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7A
•Investigate and identify properties of fluids including density, viscosity, and buoyancy
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Fluids: a substance that can flow and take shape of
its container.• Gases – can be
compressed• Liquids – diffuse
slowly (spread out evenly)
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Density of Steel
steel bar
The density of steel is the same! Size doesn’t matter! It is a ratio!
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Use the formula
sheet – you are given
the density and you can
read the volume from the cylinder!
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• Density of Water: 1.00 g/mL
• Density of Ice: 0.92 g/mL
Which one floats? Why?
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The table shows properties of four liquids that are insoluble in water. If the four liquids are poured into an Erlenmeyer flask containing water, which liquid will form a layer below the water?
A QB RC SD T
The density of water is 1
g/ml
Anything more than that will
sink!
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Boats are made so that they have a lower density
than water.
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REMINDER: Density is a ratio! As long as the
substance is the same – the density is the same!
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7D
•Relate the chemical behavior of an element including bonding, to its placement on the periodic table
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Metals
NonmetalsMetalloids
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Groups or Family Names
1) AL
KA
LI M
ET
AL
S
2) AL
KA
LIN
E
ME
TA
LS
17) HA
LO
GE
NS
18) NO
BL
E G
AS
ES
TRANSITIONMETALS
Inner earth metals
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Know the properties of the groups/families!!
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14
Silicon
(# protons) Atomic No.
Atomic Mass
Element Symbol
Atoms are Neutral: (#protons = # electrons)
Periods (across)
Groups/F
amily (dow
n)
Si 28.086
Element Name
How many protons?
How many electrons?
14
14
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A certain atom has a nucleus containing sixprotons and eight neutrons and has sixelectrons orbiting the nucleus. This atom is
aform of the element —A siliconB carbonC magnesiumD calcium
Elements are identified by the
number of protons which = the atomic
number!
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HINT: Same family = similar properties due to same # of
valence electrons
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Number of Valence Electrons
Valence Electrons:
Are electrons in the highest energy level.
The noble gases have 8 electrons.
All elements will gain, lose, or share electrons to end up with 8 electrons like the noble
gases. This is called the Octet Rule.
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Use your PTWhich of these elements is most
likely to donate one electron?F BeG CsH RnJ He
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Net Ionic ChargesMetals will lose electrons to form positive ions.
Nonmetals will gain electrons to form negative ions.
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Chemical Reactivity
• Metals increase in reactivity left and down.
• Most reactive metal is?
• Nonmetals become more reactive up and to the right.
• Most reactive nonmetal is?
Fr
F
Noble Gases are inert gases…(don’t react easily)
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How many atoms do you need?
Al3+ O2-
O2-
Al3+O2-
You need 2 Al atoms & 3 O atoms: Al2O3
Atoms will join so the sum of all
the charges = zero
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7EClassify samples of matter
from everyday life as being elements, compounds, or mixtures
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Has mass and volume (s, l, g)
More than one type of matter
Uniform throughout (solutions)
Not uniform throughout
One type of matter
One type of atom
Two or more
elements
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Properties of MatterProperty – a characteristic
Chemical properties: • characteristics of a
substance’s “ability” to change into a different substance.
• Ex. Reactivity Flamability
Physical properties:
• characteristics that can be observed or measured without changing the identity of the substance.
• Ex. Color
Density
Solubility
Melting Point
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8ADistinguish between physical and
chemical changes in matter such as oxidation, digestion, changes in states, and stages in the rock cycle
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Changes of Matter
Chemical Changes: • A change that does
produce a new substance.
• Usually not reversible.• Ex: Iron rusts forming
iron oxide.
Physical Changes:
• A change that does not produce a new substance.
• Usually reversible.
• Ex: Ice melts into water.
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How do you know a chemical change has occurred?
Evidence of aChemical Change:1. Energy (Heat):
absorbed energy (endothermic) released energy (exothermic)
2. Gas is produced (bubbles) 3. Solid (precipitate) forms 4. Odor or color change occurs
Physical change begins in the mouth
Chemical change
(Digestion) occurs in the
stomach
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Why are these chemical changes?
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The Rock CycleOne of nature’s slowest processes – the rock
cycle – is a repeating series of physical and chemical changes in which one type of rock changes to another type.
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Ice melting
Cooking
Rocks weathering
Conducts electricity
Ability to explode
Recycled aluminum can
Ability to react with acid
Burned the popcorn
Physical change
Chemical change
Physical property
Physical property
Chemical property
Physical change
Chemical property
Chemical change
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Compounds with the same chemicalcomposition may have different
densities because they —A have differences in reactivityB are able to bond with oxygenC vary in solubilityD exist in different phases
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8C
Investigate and identify the law of conservation of mass
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Law of Conservation of Mass-Mass is neither created nor
destroyed!• The total mass of the substances before they
are mixed is equal to the total mass as a mixture.
64 + 192 = 256 g Zn = 104 g
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Mass of the reactants = Mass of the products …Always!
1CH4 + 2O2 1CO2 + 2H2O1 C, 4 H, 4 O = 1 C, 4 H, 4 O
(1x12.0) + (4 x 1.0) + (4x16.0) = (1x12.0) + (4 x 1.0) + (4x16.0)
80 g = 80 gEx: How many grams of oxygen react with 16 g
of CH4 to create 80 grams of products?Reactants = Productsx g + 16 g = 80 g
x = 80-16 = 64 g O2
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CH4 (g) + O2 (g) CO2 (g) + H2O (g)
1 CH4 (g) + 2 O2 (g) 1 CO2 (g) + 2 H2O (g)
Place a coefficient in front of the compound to get the same number of atoms in the reactants
and in the products.
Count the number of atoms on both sidesof the arrow.
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Guided Practice
Ex. 1: Mg + HCl MgCl2 + H2
Ex. 2: KClO3 − KCl + O2
Balanced Equation:Mg + 2 HCl MgCl2 + H2
Balanced Equation:2 KClO3 − 2 KCl + 3 O2
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Fluids can be gases or liquids.Fluids can flow and take the shape of its container.
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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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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 theCaCO3.
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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9ARelate the structure of water
to its function as the universal solvent
Reminder: molecular structure = atomic arrangement = polar nature = polarity
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Which characteristic of water best explains its ability to dissolve a great variety of materials?
A Its transparency in lightB Its electrical conductivityC Its physical state of matterD Its molecular arrangement
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S & L
L & G
1. Phase changes require a gain or loss of ___?
2. When does it gain energy?
3. When does it lose energy?
4. At what points does the temperature stay the same?
5. Can two states coexist?
Temp is
constant
Temp is constant
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Polar Molecule:Hydrogen: Partial positive (+) charge Oxygen: Partial negative () charges.
Hydrogen BondingHydrogen and Oxygen
covalently bond to each other.
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Dissolves so many other substances due to its structure/polarity.
Positive Ion Surrounded by
oxygen ()
Negative Ion Surrounded by hydrogen (+)
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9BRelate the concentration of
ions in a solution to physical and chemical properties such as pH, electrolytic behavior, and reactivity
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Power plants that discharge warm water intorivers have a negative effect on aquatic life.This is because the higher watertemperature —
A increases the pressure of the river waterB increases the pH value of the river waterC decreases sediment solubility in the river waterD decreases the dissolved oxygen in the river water
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Nine groups of students dissolved as much potassium chloride as possible in water. Each group used 100 mL of water heated to a different temperature. Which graph shows the relationship between solubility and temperature for potassium chloride?
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“Like Dissolves Like” •You need to know that polar substances, like water, dissolve other polar substances.
•Nonpolar substances dissolve nonpolar substances
•Put a nonpolar substance and a polar substance together and you will find that they don’t mix! Like oil and water.
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Solutions• Solution – Solution – a homogeneous mixture
SolventSolvent – substance doing the dissolving
SoluteSolute - substance being dissolved
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Dissolving RateIncrease rate of dissolving by:• Stirring or Shaking (moves molecules
around)• Crushing or grinding (increases
surface area)• Heating (increases movement of
molecules)
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More solvent than solute. Ex. Lightly
sweetened
Solvent has dissolved all the
solute it can hold. Ex. Sweet tea
Solvent holds more solute than is normal.
Ex. Rock candy
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Solubility Curves
Look at KNO3• Point on the line
= Saturated• Point below the
line = Unsaturated
• Point above the line = Supersaturated
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Solubility increases as the temperature increases for most substances (upward
curves)
Example: Dissolve sugar in hot tea vs. iced tea
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Example: Soda pop What happens when you leave a soda out on a hot day?
Carbon dioxide gas will go out as the soda
warms up making it flat.
Solubility of gases in water decreases with increasing temperature.
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Pressure & Gases
Solubility of liquids and solids isn’t affected much.
Gas solubility ALWAYS increases as pressure increases.
The way to get gas to dissolve in liquid is to pressurize the mixture, meaning that the pressure inside a soda can is greater than the pressure outside the can.
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Increase PressureDecrease Volume
Increase TemperatureIncrease Volume
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Non-electrolyte: (ex. pure water) No ions present,
thus, no electrical conductivity.
Weak electrolyte: (ex.weak acid/base) Few ions present,
thus, poor electrical conductivity.
Strong electrolyte: (ex. Strong acid/base)
Salt completely breaks apart to give more ions,
conduct more electricity.
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Bases are:
• pH more than 7
•Bitter and Slippery
•Change Red litmus paper will to blue.
•Forms Hydroxide ions.
Acids are:
• pH less than 7
•Sour, like lemons
•Change Blue litmus paper to red.
•Forms Hydrogen ions
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Now You Try!Now You Try!Now You Try!Now You Try!
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The bonding characteristics of oxygen aremost similar to the bonding characteristicsof —A hydrogenB siliconC heliumD sulfur