First Semester Exam Review

First Semester Exam ReviewPhysical Science2013 Exam Schedule:Tuesday, Dec. 17: 1st & 3rd Wednesday, December 18: 5th & 7th Thursday, December 19: 2nd & 4th Friday, December 20: 6th & 8thExams are 25% of the semester grade!

Calculation: Sem. Grade = (0.75)(18-wk.avg.) + (0.25)(Exam)

Exam = Desired Sem. Grade (0.75)(18-wk. avg.) 0.25

1Experimental DesignYou will be given an experiment in which you must identify the following components.Independent Variable You change it.Dependent Variable - It changed.Constants variables that remain the sameControl does not receive the treatmentSignificant FiguresDetermining # of Sig. Fig. examples:Sig. Figs in Calculations:1) 10000 = 1 sig. fig.2) 10001 = 5 sig. figs3) 10000. = 5 sig. figs4) 10000.0 = 6 sig. figs5) 0.0001 = 1 sig. fig.6) 0.00010 = 2 sig. figs7) 0.000101 = 3 sig. figs8) 10.00010 = 7 sig. figsAddition and Subtraction: 5.687 g -2.31g = 3.377 g = 3.38 g (rounded to 2 decimal places)

Multiplication and Division:(12.500 cm)(2.00 cm) = 25.0cm2Scientific NotationWrite 59000000 m in scientific notation. 5.9 x 107 m This shows 2 sig. figs. If you needed to round to 1 sig. fig. : 6 x 107 m

Write 0.0000256 m in scientific notation. 2.56 x 10-5 m (rounded to 3 sig. figs) If you need to round to 2 sig figs: 2.6 x 10-5 m If you need to round 1 sig. figs: 3 x 10-5 m Scientific NotationConvert the following to Scientific Notation:

1,870,000 m320,000,0000.000 000 005 6 kg0.000 987Scientific NotationConvert the following to Scientific Notation:

1,870,000 m= 1.87 x 106 m320,000,000= 3.2 x 1080.000 000 005 6 kg= 5.6 x 10-9 kg0.000 987= 9.87 x 10-4Dimensional Analysis Kilo- Hecto- Deca- Basic unit (m, l, g) deci- centi- milli-

Convert 45.000 km to m 45.000 km x 1000m = 45,000 m 1 kmConvert 2000 cm to m 2000 cm x 1m = 20 m 100 cmConvert 500000 mm to km500000 mm x _1 km = 0.5 km 106 mmDimensional Analysis Problems3.50 kg to g0.50 cg to mg120.50 g to kg0.0500 kg to mgCheck your work:a) 3.50 kg x 1000 g = 3500 g 1 kgb) 0.50 cg x 10 mg = 5 mg

c) 120.50 g x _1kg___ = 0.1205 kg 1000 g

d) 0.0500 kg x 106 mg = 5.00 x 104 mg 1 kgVolumeSolid rectangular object:

The volume of an irregularly-shaped object can be determined through the water-displacement method:

What is the volume of the object?The volume of an irregularly-shaped object can be determined through the water-displacement method:

What is the volume of the object?

75 mL 50 mL = 25 mL

The volume of the object is 25 mL. The object occupies 25 mL of volume.

Density D = m v

V = m D

M = D x v

Objects with a density greater than waters density, which is 1.00 g/mL, will sink in water, while objects with a density less than waters will float in water. Temperature affects density. Since matter tends to expand when heated and contract when cooled, the density decreases with increasing temperature, and increases with decreasing temperature.

Density Problem:a) The density of silver (Ag) is 10.5 g/cm3. Find the mass of Ag that occupies 965 cm3 of space. Density Problem Solution:The density of silver (Ag) is 10.5 g/cm3. Find the mass of Ag that occupies 965 cm3 of space. D = m (solve for m) vD = 10.5 g/cm3 m = D vm= ? m = (10.5 g/cm3)(965 cm3)v = 965 cm3 m = 10,132.5 g

Density Problem:b) A 2.75 kg sample of a substance occupies a volume of 250.0 cm3. Find its density in g/cm3.

Density Problem Solution:b) A 2.75 kg sample of a substance occupies a volume of 250.0 cm3. Find its density in g/cm3. D = mD = ? vm = 2.75 kg D = 2750 g2.75 kg x 1000g = 2750 g 250.0 cm3 1 kg v = 250.0 cm3 D = 11 g/cm3

Density Problem:c) Under certain conditions, oxygen gas (O2) has a density of 0.00134 g/mL. Find the volume occupied by 250.0 g of O2 under the same conditions. Density Problem Solution:c) Under certain conditions, oxygen gas (O2) has a density of 0.00134 g/mL. Find the volume occupied by 250.0 g of O2 under the same conditions. v = m D D = 0.00134 g/mLm = 250.0 gv = 250.0 gv = ?0.00134 g/mLv = 18,656 mLKinetic Theory of Matter and States of Matter

Kinetic Theory: all matter is made up of tiny particles in constant motion. More motion among particles (increase in KE), temperature increases, and the changes in state of matter occur.

Temperature is the measure of the average kinetic energy (KE) of the particles that make up matter.

20Boyles Law

When temperature is held constant, volume and pressure are inversely proportional. P1V1 = P2V2

At constant temperature, as the volume decreases, the particle speed increases, so the number of collisions with the walls of the container increases, therefore the pressure also increases.As volume increases, particle motion slows, collisions with the walls of the container decrease, & pressure decreases.Charles LawWhen pressure is held constant, volume and temperature and are directly proportional. V1 = V2 T1 T2

As particle speed increases, temperature increases, and the particles expand, so the volume increases.

Chemical or Physical? boiling of waterbursting of a ballooncrumpling paperburning of gasolinerotting of an eggexploding fireworks23 Chemical or Physical? boiling of water Pbursting of a balloon Pcrumpling paper Pburning of gasoline Crotting of an egg Cexploding fireworks C24Chemical or Physical? freezing of waterevaporation of gasolinerusting a nailsawing of wood crushing a can toasting a marshmallow

25Chemical or Physical? freezing of water Pevaporation of gasoline Prusting a nail Csawing of wood Pcrushing a can Ptoasting a marshmallow C

26According to the law of conservation of mass, how does the mass of the products in a chemical reaction compare to the mass of the reactants?a. There is no relationship.b. The mass of the products is greater.c. The mass of the reactants is greater.d. The masses are equal.27Ten Signs of Chemical Change

Bubbles of gas appear. (double replacement rxn.)A precipitate forms. (a solid falls out of solution when 2 aqueous solutions react usually in double replacement reactions)A color change occurs.The temperature changes.Light is emitted.

Ten Signs of Chemical Change (cont.)A change in volume occurs.A change in electrical conductivity occurs.A change in melting point or boiling point occurs.A change in odor or taste occurs. A change in any distinctive chemical or physical property occurs.

Determine the number of protons, neutrons and electrons in a given element. Ex. Uranium-238

Determine the number of protons, neutrons and electrons in a given element. Ex. Uranium-23892 protons, 146 neutrons, 92 electrons

Calculate the average atomic mass of silver if 51.48% of its atoms have a mass of 106.905 amu and 48.17% of its atoms have a mass of 108.905 amu.

(0.5148)(106.905 amu) = 55.034 amu(0.4817)(108.905 amu) = +52.460 amu 107.494 amu

At room temperature, most metals are ____.radioactivegasesliquidssolids

34Group 1 elements are called the ________________________.

What makes this group highly reactive?Group 1 elements are called the alkali metals

What makes this group highly reactive?The alkali metals are highly reactive because they all have one valence electron. An atom needs a full valence shell, like a Noble Gas, to be stable and unreactive.Why is hydrogen is grouped with the alkali metals?

Why is hydrogen is grouped with the alkali metals?

Hydrogen has one valence electron, as do the alkali metals (group 1).What do elements in the same group have in common?

What do elements in the same period have in common?What do elements in the same group have in common? same # of valence electrons

What do elements in the same period have in common? same # of energy levelsWhat is the relationship between the elements sodium and potassium?

What is the relationship between the elements sodium and potassium?

They are both alkali metals in group 1 and they both have 1 valence electron.

Which statement is true of the elements sodium and potassium?a. They are polyatomic ions.b. They are compounds.c. They are nonmetals.d. They are metals.43The properties of sodium and potassium are:a.quite different because they have different electron arrangements

b.quite different because they have similar electron arrangements

c.quite similar because they have different electron arrangements

d.quite similar because they have similar electron arrangements4420. Which of the statements below is true of the elements sodium and potassium?a. they form the compound NaK

b. they have very different chemical properties

c. belong to the same period

d. belong to the same group (family)

45Why are the atomic masses of the elements not whole numbers?

Why are the atomic masses of the elements not whole numbers?

Each element has various isotopes that are present in nature, and theatomic massis a weighted average of all of the isotopes that occur naturally. Atomic masses are calculated using the percent abundance and mass of each of its isotopes.

IsotopesAtoms of the same element that have different numbers of neutrons, and thus, different masses.All Isotopes of carbon all have 6 protons.Carbon -12 = 6 protons + 6 neutronsCarbon -13 = 6 protons + 7 neutronsCarbon -14 = 6 protons + 8 neutrons

Bohr Model

K = 2 e-L = 8 e-M = 18 e-N = 32 e-

Identify this element.A: BoronKnow the Bohr models of elements 1-20.Lewis Dot Diagrams show only valence electrons

Be able to determine the correct Lewis dot diagram for a given element. (Look @ group # for a hint).Properties of MetalsLustershiny, reflect lightConduct (carry) Heat Conduct electricity (silver is a better conductor than copper, but silver is more expensive, so copper is used)Ductilethe ability to be drawn into thin wiresMalleablecan be flattened into thin sheets without shattering or crumblingAll are solids at room temperature except Mercury-(liquid)Location on the periodic table: left side of the stair-step line (see previous slide)

Properties of NonmetalsLack luster (not shiny)Poor conductors of heat and electricityNot ductileNot malleable, most nonmetal solids will crumble if hammeredExist as solids, liquids, and gasesMany of the nonmetals exist as diatomic gases (Br2, I2, N2, Cl2, H2, O2, F2)Location on the periodic table: to the right of the stair-step line.

MetalloidsAlso known as semi-metals or semi-conductorsLie along the stair-step LineExhibit properties of both metals and nonmetalsWhat is a cation?

How does a cation form?

What kinds of elements tend to form cations?What is a cation? a positive ion (+)

How does a cation form? A cation forms when an atom loses one or more electrons.

What kinds of elements tend to form cations? metalsWhat is an anion?

How does an anion form?

What kinds of elements tend to form anions? nonmetalsWhat is an anion? a negative ion (-)

How does an anion form?An anion forms when atom gains one or more electrons.

What kinds of elements tend to form anions? nonmetalsWhat kind of chemical bond is formed when an equal exchange of electrons occurs?a. hydrogenb. magneticc. covalentd. ionic58The ________________________ tells you how many electrons an atom must gain, lose, or share to become stable.

The oxidation number tells you how many electrons an atom must gain, lose, or share to become stable.

The oxidation number of an atom is shown with a __________________________.

The oxidation number of an atom is shown with a superscript.

The sum of the oxidation numbers in a neutral compound is alwaysnegative positive onezero63Types of BondsWhat kind of chemical bond is formed when an equal exchange of electrons occurs?

What kind of bond forms when atoms share electrons?

What kind of chemical bond is formed when an equal exchange of electrons occurs? ionic bond

What kind of bond forms when atoms share electrons? covalent bond

How an ionic bond forms

Sodium loses its one valence electron, becoming the sodium ion, Na1+The chlorine atom gains the electron from sodium to form the chloride ion, Cl1-.Ionic bond is an electrostatic attraction between ions.In a chemical formula, the number of each type of atom in the compound is shown by numbers called ____.

In a chemical formula, the number of each type of atom in the compound is shown by numbers called subscripts.

Compare and Contrast Ionic vs. Covalent BondsIonic BondsGain or lose electrons (an equal exchange of electrons)Metal + Nonmetal (usually)Usually solidsStronger bond (high melting point)

Covalent BondsShare valence electronsNonmetal + NonmetalUsually gases or liquidsWeaker bond (lower melting point)

What is the correct formula for magnesium oxide?

Mg2O Mg2O2 MgO2 MgO 70What is the correct formula for magnesium oxide?

Mg2O Mg2O2 MgO2 MgO 71In a chemical formula, the number of each type of atom in the compound is shown by numbers called ____.superscriptsoxidation numberschemical symbolssubscripts72The oxidation number of an atom is shown with a ___.a. negative number b. subscript c. positive numberd. superscript73How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?246874Why do the noble gases NOT form compounds readily?a.They have empty outer energy levels.b.They have no electrons.c.They have seven electrons in the outer energy levels.d.Their outer energy levels are completely filled with electrons. 75What is the name of a binary compound made up of lithium and chlorine?a. chlorine lithiateb. lithium chloratec. chlorine lithiumd. lithium chloride76Hydrogen is grouped with the alkali metals because it is a metal is a gasdoes not readily form compoundshas one electron in its outer energy level

77How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2?a. 4b. 3c. 12d. 778The ____ tells you how many electrons an atom must gain, lose, or share to become stable.a. atomic massb. ionic numberc. atomic numberd. oxidation number79What is the charge of phosphate in K3PO4?a. 7-b. 1+c. 4+d. 3-80What is the name of CaBr2?calcium (II) bromidecalcium bromatecalcium (II) bromatecalcium bromide81What is the formula for copper(II) chloride?a. CClb. Cu2Clc. CuCld. CuCl282What is the name of PbO2?lead oxalatelead dioxidelead (II) oxidelead (IV) oxide

83What is the formula for magnesium chloride?MgClMnClMnCl2MgCl284The formula for iron (III) chloride isa. FeClb. FeClO3c. Fe3Cld. FeCl385The formula for calcium phosphate is:a. CaPO4b. Ca3PO4c. Ca3P2d. Ca3 (PO4)286AnswersThe answers to every multiple choice question in this slideshow is D.Know the polyatomic ions:Here are a few basic ones to know1. phosphate ion

2. carbonate ion

3. nitrate ion

4. sulfate ion

5. ammonium ion

A. NO3-B. SO42-C. NH4+D. PO43-E. CO32-

88Know the polyatomic ions:D 1. phosphate ion E 2. carbonate ion

A 3. nitrate ion

B 4. sulfate ion

C 5. ammonium ionA. NO3-B. SO42-C. NH4+D. PO43-E. CO32-

89Write formulas for the following ionic compounds.a) copper (II) chlorideb) magnesium iodidec) iron (III) bromided) tin (IV) chlorideCheck your work:a) copper (II) chloride = CuCl2b) magnesium iodide = MgI2c) iron (III) bromide = FeBr3d) tin (IV) chloride = SnCl4Write formulas for the following ionic compounds.e) calcium phosphate

f) sodium nitrite

g) iron (III) sulfate

h) lead (IV) oxideCheck your work:e) calcium phosphate = Ca3(PO4)2

f) sodium nitrite= NaNO2

g) iron (III) sulfate=Fe2(SO4)3

h) lead (IV) oxide= PbO2Write names for the following compounds:PbOPbO2NH4ClCaCl2Check your work:PbO = lead (II) oxidePbO2= lead (IV) oxideNH4Cl= ammonium chlorideCaCl2= calcium chlorideWrite names for the following compounds:e) FeOf) Fe2O3g) Mg(NO3)2 h) Ca3(PO4) 2Check your work:e) FeO=iron (II) oxidef) Fe2O3=iron (III) oxideg) Mg(NO3)2 =magnesium nitrateh) Ca3(PO4)2= calcium phosphateThe name for a single unit of a covalent compound is a _____.

A single unit of an ionic compound is called a _______.The name for a single unit of a covalent compound is a molecule.

A single unit of an ionic compound is called a formula unit.MORE ACTICE WITH WRITING CHEMICAL FORMULAS & NAMING COMPOUNDSWrite the formula from the following names:

a) copper(II) chlorideb) lithium bromidec) zinc oxide d) zinc nitridee) zinc chloride

Answersa) copper(II) chloride = CuCl2b) lithium bromide= LiBrc) zinc oxide = ZnOd) zinc nitride = Zn3N2e) zinc chloride = ZnCl2Write the formula from the following names:

f) barium chlorideg) iron (II) sulfideh) magnesium sulfatei) sodium phosphatej) iron (II) oxide

Answersf) barium chloride = BaCl2g) iron (II) sulfide = FeSh) magnesium sulfate = MgSO4i) sodium phosphate = Na3PO4j) iron (II) oxide = FeOWrite the formula from the following names:

k) iron (III) oxidel) magnesium phosphidem) calcium phosphate n) lead (II) chlorideo) nickel III) chloride

Answersk) iron (III) oxide = Fe2O3l) magnesium phosphide = Mg3P2m) calcium phosphate = Ca3(PO4) 2n) lead (II) chloride = PbCl2o) nickel III) chloride = NiCl3Write names from the formulas given:

a) PbO b) PbO2c) Zn3(PO4)2d) Cu(HCO3)2e) FeSO4 Answers:PbO = lead (II) oxide PbO2 = lead (IV) oxideZn3(PO4)2 = zinc phosphateCu(HCO3)2 = copper (II) bicarbonateFeSO4 = iron (II) sulfateWrite names from the formulas given: f) NaHCO3 g) CuCl h) CuCl2 i) K2SO4 j) Al2O3Answers: f) NaHCO3 = sodium bicarbonate g) CuCl = copper (I) chloride h) CuCl2 = copper (II) chloride i) K2SO4 = potassium sulfate

j) Al2O3 = aluminum oxideWrite names from the formulas given:k) Fe2O3l) NiO

m) Ni2O3 n) MnO2o) Cr2O3BEFORE EXAMS:Dont wait until the last minute to study!Study a little for each exam each day!Use the online resources available to you on my TeacherWeb site. There are PowerPoints under Handouts and online quizzes you may take.Use your smartphone to review the PowerPoints.Get a good nights rest each night! (8+ hours)Eat right! Junk will make you feel tired. Nothing too heavy for breakfast!Research shows that water increases your brain power, so drink plenty of it!For multiple choice items, eliminate impossible answers! As always, I am available for help.My email: nkfox@caddo.k12.la.us