Chapter 12 Review- Chemical Periodicity. Chapter 12 Review - definitions electronegativity electronegativity periods periods atomic radius atomic radius

Chapter 12 Review-Chapter 12 Review-Chemical PeriodicityChemical Periodicity

Chapter 12 Review - Chapter 12 Review - definitionsdefinitions

electronegativityelectronegativity periodsperiods atomic radiusatomic radius ionization energyionization energy periodic tableperiodic table


alkali metalsalkali metals halogenshalogens noble gasesnoble gases alkaline earth metalsalkaline earth metals groupsgroups

Chapter 12 ReviewChapter 12 Review

The modern periodic table is The modern periodic table is arranged in order of increasing:arranged in order of increasing:

The elements in Groups 1A through The elements in Groups 1A through 7A and Group 0 make up the:7A and Group 0 make up the:

What are characteristics of the noble What are characteristics of the noble gases?gases?

( atomic number )

( representative elements )

( outer s and p sublevels filled, belong to Group 0, called inert gas )


What is the number of electrons in What is the number of electrons in the outermost occupied energy the outermost occupied energy level of an element in Group 5A?level of an element in Group 5A?

Which have the same number of Which have the same number of electrons in their outermost energy electrons in their outermost energy levels? a) K, Ca, Rb, Sr b) N, P, As, levels? a) K, Ca, Rb, Sr b) N, P, As, SbSb

( 5 )

( b )


An element that contains an electron An element that contains an electron in a in a dd sublevel is: a) Mg b) Fe sublevel is: a) Mg b) Fe

The elements that contain electrons The elements that contain electrons in the in the ff sublevels are referred to as: sublevels are referred to as:

The outermost energy level The outermost energy level configuration of the element chlorine configuration of the element chlorine is:is:

( b )

( inner transition metals )

( 3s23p5 )


The element with 8 electrons in its The element with 8 electrons in its 3d sublevel is: a) Ar b) Ni3d sublevel is: a) Ar b) Ni

As you move down a group of the As you move down a group of the periodic table, atomic size periodic table, atomic size generally:generally:

The largest atom from among the The largest atom from among the following is: a) Fr b) Rbfollowing is: a) Fr b) Rb

( b )

( increases )

( a )


The smallest atom from the The smallest atom from the following is: a) Cl b) Sifollowing is: a) Cl b) Si

As the number of electrons added to As the number of electrons added to the same principal energy level the same principal energy level increases, atomic size generally:increases, atomic size generally:

Removing one electron from a Removing one electron from a gaseous atom forms a:gaseous atom forms a:

( Cl )

( decreases )

( 1+ ion )

Chapter 12 ReviewChapter 12 Review Among the elements listed, which Among the elements listed, which

would show the largest increase would show the largest increase between the 2nd and 3rd ionization between the 2nd and 3rd ionization energies? a) Ca b) Znenergies? a) Ca b) Zn

Among the following, which element Among the following, which element has the lowest IE? a) Cs b) Ihas the lowest IE? a) Cs b) I

Among the following, which has the Among the following, which has the highest 2nd IE? a) Na b) Clhighest 2nd IE? a) Na b) Cl

( a )

( a )

( a )


Which of the following are always Which of the following are always larger than the neutral atoms from larger than the neutral atoms from which they are formed? a) which they are formed? a) cations b) anionscations b) anions

The smallest particle from among The smallest particle from among the following is: a) Li b) Lithe following is: a) Li b) Li1+1+

Which is the least electronegative? Which is the least electronegative? a) S b) Cs a) S b) Cs

( b )

( b )

( b )

Element Period No. Group No. Group Name Symbol

Fill in requested information from given:

2s2

3s23p3

3s23p6

4s1

4s23d1

4s24p5

( 2 ) ( 2A ) ( alkaline earth metal) ( Be )

( 3 ) ( 5A ) (representative element) ( P )

( 3 ) ( 0 ) ( noble gas ) ( Ar )

( 4 ) ( 1A ) ( alkali metal ) ( K )

( 4 ) ( 3B ) ( transition metal ) ( Sc )

( 4 ) ( 7A ) ( halogen ) ( Br )


Arrange the following: Li, C, K, Arrange the following: Li, C, K, F, CsF, Cs decreasing atomic size:decreasing atomic size:

increasing ioniztion energy:increasing ioniztion energy:

decreasing electronegativity:decreasing electronegativity:

( Cs, K, Li, C, F )

( Cs, K, Li, C, F )

( F, C, Li, K, Cs )


Atom Larger Greater Ionization Energy Lower Electronegativity

Li, K

C, F

Mg, Ca

O, S

( K ) ( Li ) ( K )

( C ) ( F ) ( C )

( Ca ) ( Mg ) ( Ca )

( S ) ( O ) ( S )


Explain why atoms with high Explain why atoms with high ionization energies typically ionization energies typically also have high also have high electronegativities.electronegativities. ( A high ionization energy indicates that an atom has a tight hold on it’s electrons. A high electronegativity indicates an ability to attract additional electrons. They both refer to a desire to have electrons. )

Chapter 17 ReviewChapter 17 Review“Reaction Rates and Equilibrium”“Reaction Rates and Equilibrium”

Chapter 17 ReviewChapter 17 Review Energy that is Energy that is availableavailable to do work to do work

is called ____.is called ____. ____ is defined as the number of ____ is defined as the number of

atoms, ions, or molecules that atoms, ions, or molecules that react react in a given timein a given time to form products. to form products.

What is the name of the What is the name of the minimum minimum energyenergy that colliding particles must that colliding particles must have in order to react?have in order to react?

Free energy

Reaction Rate

Activation Energy

Chapter 17ReviewChapter 17Review A substance that A substance that interferesinterferes with a with a

catalyst is a(n) ____.catalyst is a(n) ____. What is the arrangement of atoms What is the arrangement of atoms

at the at the peakpeak of an energy barrier? of an energy barrier? At At equilibriumequilibrium, what is the rate of , what is the rate of

production of reactants compared production of reactants compared with the rate of production of with the rate of production of products?products?

inhibitor

Activated complex

The same

Chapter 17 ReviewChapter 17 Review What is the equilibrium constant What is the equilibrium constant

expressionexpression for the following reaction: for the following reaction: CC(s)(s) + O + O2(g)2(g) ↔ CO↔ CO2(g)2(g)

Which of the following is Which of the following is true true about the about the combustion of carbon: a) the reaction is combustion of carbon: a) the reaction is spontaneous, or b) entropy decreases?spontaneous, or b) entropy decreases?

The rate of a chemical reaction normally The rate of a chemical reaction normally ____ as reactant ____ as reactant concentration concentration increasesincreases..

[Carbon Dioxide]

[Carbon] [Oxygen]

a

increases

Chapter 17 ReviewChapter 17 Review Why does a higher concentration Why does a higher concentration

make a reaction make a reaction fasterfaster?? The amount of The amount of disorderdisorder in a system in a system

is measured by its ____.is measured by its ____. EntropyEntropy measures ____ measures ____ For a For a complex reactioncomplex reaction, the reaction , the reaction

progress curve has several ____.progress curve has several ____.

More collisions /time

entropy

disorder

Elementary steps

Chapter 17 ReviewChapter 17 Review What happens to a reaction at What happens to a reaction at

equilibrium when equilibrium when more reactantmore reactant is is added to the system?added to the system?

Which reaction results in the greatest Which reaction results in the greatest increaseincrease in entropy: in entropy: a) A a) A → B, or b) A → 2B→ B, or b) A → 2B

If a reaction has an equilibrium constant If a reaction has an equilibrium constant (K(Keqeq) just ) just greater than 1greater than 1, how do we , how do we

interpret that information?interpret that information?

The Reaction shifts to the right

b

The Reaction slightly favorsProducts at equilibrium

Chapter 17 ReviewChapter 17 Review A A catalystcatalyst works by ____. works by ____. If sulfur dioxide and oxygen can be If sulfur dioxide and oxygen can be

made into sulfur trioxide, what is the made into sulfur trioxide, what is the reversereverse reaction? reaction?

Which variable is Which variable is NOTNOT required to required to calculate the Gibbs free-energy calculate the Gibbs free-energy change for a chemical reaction: change for a chemical reaction: a) change in enthalpy, or a) change in enthalpy, or b) temperature in b) temperature in ooC?C?

Lowering the activation energy barrier

SO3 S + O2

b

Chapter 17 ReviewChapter 17 Review What is the effect of What is the effect of adding more adding more

waterwater to the following equilibrium to the following equilibrium reaction: COreaction: CO22 + H + H22O O ↔ H↔ H22COCO33

In an endothermic reaction at In an endothermic reaction at equilibrium, what is the effect of equilibrium, what is the effect of raising the temperatureraising the temperature??

The energy that is The energy that is availableavailable to do to do work in a reaction is called ____.work in a reaction is called ____.

Shift right

Shift Right

Free energy

Chapter 17 ReviewChapter 17 Review What is the numerical value (+ or -) What is the numerical value (+ or -)

of Gibbs free-energy change for a of Gibbs free-energy change for a spontaneousspontaneous reaction? reaction?

Which of the following systems has Which of the following systems has the the highest entropyhighest entropy: : a) 10 mL of water at 50 a) 10 mL of water at 50 ooC, or C, or b) 10 mL of water at 100 b) 10 mL of water at 100 ooC? C?

negative

b

Chapter 17 ReviewChapter 17 Review What happens to a What happens to a catalystcatalyst in a in a

reaction?reaction? Write the Write the rate lawrate law for the following for the following

reaction: A + 2B reaction: A + 2B → C + D→ C + D An An elementaryelementary reaction converts reaction converts

reactants to products in ____.reactants to products in ____. Activation energyActivation energy is ____. is ____. Is the Is the melting of icemelting of ice at a temperature at a temperature

above 0 above 0 ooC: C: a) endothermic, or b) exothermic?a) endothermic, or b) exothermic?

The catalyst remains nchanged

Rate = k[A][B]2

One step

The energy needed to make reactantsBecome products

a

Chapter 17 ReviewChapter 17 Review Consider the reaction: Consider the reaction:

N N2(g)2(g) + 3H + 3H2(g)2(g) ↔ 2NH↔ 2NH3(g)3(g)

What is the effect of What is the effect of decreasing the decreasing the volumevolume on the contained gases? on the contained gases?

Spontaneous reactionsSpontaneous reactions always ____ always ____ free energy.free energy.

Why does a Why does a higher temperaturehigher temperature cause a reaction to go faster?cause a reaction to go faster?

Shift right

release

Increases the likelyhood of a successful collision

Chapter 17 ReviewChapter 17 Review What What 2 factors2 factors determine whether determine whether

or not a reaction is spontaneous?or not a reaction is spontaneous?

What What physical statephysical state of nitrogen has of nitrogen has the highest entropy?the highest entropy?

What is another name for the What is another name for the catalysts catalysts in your bodyin your body??

Increasing entropy and decreasing enthalpy

gas

enzyme

Chapter 17 ReviewChapter 17 Review What is the What is the orderorder of the following of the following

reaction: A + 2B reaction: A + 2B → C + D→ C + D Why does a catalyst cause a reaction to Why does a catalyst cause a reaction to

proceed fasterproceed faster?? In an equilibrium reaction with a In an equilibrium reaction with a KKeqeq of 1 of 1

x 10x 1088, the ____ are favored., the ____ are favored. Which of the following explains why Which of the following explains why

melting of ice is melting of ice is spontaneousspontaneous at room at room temperature and pressure: temperature and pressure: a) it is accompanied by an increase in a) it is accompanied by an increase in entropy, or b) it is accompanied by an entropy, or b) it is accompanied by an increase in energy?increase in energy?

3rd order

Lower activation energy barrier

products

a

Chapter 17 ReviewChapter 17 Review The The KKeqeq of a reaction is 4 x 10 of a reaction is 4 x 10-7-7. At . At

equilibrium, the ____ are favored.equilibrium, the ____ are favored. Another name for the Another name for the activated activated

complexcomplex is ____. is ____. Which change would shift the Which change would shift the

following reaction following reaction to the rightto the right: : 4HCl4HCl(g)(g) + O + O2(g)2(g) ↔ 2Cl↔ 2Cl2(g)2(g) + 2H + 2H22OO(g)(g) a) a) decrease of pressure, or b) decrease of pressure, or b) increase of pressure?increase of pressure?

reactants

Transition state

b

Chapter 17ReviewChapter 17Review In which of these systems is the In which of these systems is the

entropy decreasingentropy decreasing: : a) salt dissolving in water, or a) salt dissolving in water, or b) a liquid cooling?b) a liquid cooling?

Given: 2NClOGiven: 2NClO(g)(g) ↔ 2NO↔ 2NO(g)(g) + Cl + Cl2(g)2(g) An analysis of the equilibrium An analysis of the equilibrium mixture in a 1 L flask is: NClO = 1.6 mixture in a 1 L flask is: NClO = 1.6 mol; NO = 6.4 mol; Clmol; NO = 6.4 mol; Cl22 = 0.49 mol. = 0.49 mol. Calculate the value of KCalculate the value of Keqeq..

b

7.84

Chapter 17 ReviewChapter 17 Review In a In a two-step reactiontwo-step reaction mechanism, mechanism,

how many elementary reactions how many elementary reactions occur?occur?

The KThe Kspsp of calcium hydroxide is of calcium hydroxide is

6.5 x 106.5 x 10-6-6. If the concentration is . If the concentration is 0.0010 M Ca(OH)0.0010 M Ca(OH)22, what is the , what is the

final final concentration of the calcium concentration of the calcium ionion??

2

2.4x10-3

Chapter 17 ReviewChapter 17 Review A mixture of hydrogen and iodine A mixture of hydrogen and iodine

are in equilibrium with hydrogen are in equilibrium with hydrogen iodide, as shown in the equation: iodide, as shown in the equation:

HH22 + I + I22 ↔ 2HI↔ 2HI

Calculate the concentration of HICalculate the concentration of HI when the Kwhen the Keqeq is 1 x 10 is 1 x 1055, the , the

equilibrium concentration of Hequilibrium concentration of H22 is is

0.04 M, and the equilibrium 0.04 M, and the equilibrium concentration of Iconcentration of I22 is 0.009 M. is 0.009 M.

6 x 10 -5


Chapter 18 Review Chapter 18 Review Acids and BasesAcids and Bases


acidic solutionacidic solution conjugate acid-base pairconjugate acid-base pair amphotericamphoteric alkaline solutionalkaline solution KKww


hydroxide ionhydroxide ion neutral solutionneutral solution hydronium ionhydronium ion KKaa

triprotic acidtriprotic acid


A solution in which the hydroxide A solution in which the hydroxide ion concentration is 1 x 10ion concentration is 1 x 10-5-5 M is: M is:

In a neutral solution, the [ HIn a neutral solution, the [ H1+1+ ] ] is:is:

( basic )

( equal to [ OH1- ] )


What are the products of the self What are the products of the self ionization of water?ionization of water?

Which is most basic: a) [ HWhich is most basic: a) [ H++ ] = 1 ] = 1 x 10x 10-11-11, or b) [ OH, or b) [ OH-- ] = 1 x 10 ] = 1 x 10-4-4??

The formula of the hydrogen ion The formula of the hydrogen ion is often written as:is often written as:

( OH- and H+ )

( a )

( H+ )


What is the pH of a solution in What is the pH of a solution in which the [ Hwhich the [ H++ ] = 1 x 10 ] = 1 x 10-12-12??

What is the pH of a 0.01 M What is the pH of a 0.01 M hydrochloric acid solution?hydrochloric acid solution?

If KIf Kaa for H for H22COCO33 is 4.3 x 10 is 4.3 x 10-7-7, it , it means that Hmeans that H22COCO33 is: is:

( 12.0 )

( 2.0 )

( a poor hydrogen-ion donor )


Which of the following pairs Which of the following pairs consist of a weak acid and a consist of a weak acid and a strong base? a) ethanoic acid, strong base? a) ethanoic acid, sodium hydroxide or b) sulfuric sodium hydroxide or b) sulfuric acid, sodium hydroxideacid, sodium hydroxide( a )


In the reaction NHIn the reaction NH441+1+ + H + H22O O

NHNH33 + H + H33OO1+1+, water is acting as , water is acting as a(n):a(n):

A solution with a pH of 5.0:A solution with a pH of 5.0:

( Bronsted-Lowry base )

( has a hydroxide ion concentration of 1 x 10-9 M )


With solutions of strong acids With solutions of strong acids and strong bases, the word and strong bases, the word strongstrong refers to: refers to:

Which of these is an Arrhenius Which of these is an Arrhenius base? a) KOH, or b) NHbase? a) KOH, or b) NH33??

( the degree of ionization )

( a )


Ethanoic acid ionizes in water as:Ethanoic acid ionizes in water as:

CHCH33COOH + HCOOH + H22O CHO CH33COOCOO1-1- + H + H33OO1+1+

The ethanoate ion (CHThe ethanoate ion (CH33COOCOO1-1-) is ) is therefore:therefore:

1%

--><--

99%

( a good hydrogen-ion acceptor )


Which acid is monoprotic?Which acid is monoprotic?

a) CHa) CH33COOH, or b) HCOOH, or b) H22COCO33

A 12.0 M solution of an acid that A 12.0 M solution of an acid that is able to ionize completely in is able to ionize completely in solution would be termed:solution would be termed:

( a )

( concentrated and strong )


According to the Bronsted-Lowry According to the Bronsted-Lowry theory, water will act as a base theory, water will act as a base when it:when it:

( accepts a hydrogen ion )


What are the Bronsted-Lowry What are the Bronsted-Lowry acids in this equilibrium acids in this equilibrium reaction?reaction?

CNCN1-1- + H + H22O O HCN + OH HCN + OH1-1-

( H2O and HCN )


Calculate the pH, and state if it is Calculate the pH, and state if it is an acid, base, or neutral solution:an acid, base, or neutral solution:

[ H[ H++ ] = 1 x 10 ] = 1 x 10-9-9

[ OH[ OH-- ] = 1 x 10 ] = 1 x 10-10-10

[ OH[ OH-- ] = 1 x 10 ] = 1 x 10-1-1

[ H[ H++ ] = 1 x 10 ] = 1 x 10-7-7

( pH = 9; it is basic )

( pH = 4; it is acidic )

( pH = 13; it is basic )

( pH = 7; it is neutral )


Calculate the hydrogen-ion Calculate the hydrogen-ion concentration [ Hconcentration [ H++ ] for an ] for an aqueous solution in which [ OHaqueous solution in which [ OH-- ] ] is 1 x 10is 1 x 10-12-12 mol/L. Is this solution mol/L. Is this solution acidic, basic, or neutral?acidic, basic, or neutral?

( [ H+ ] = 1 x 10-2; it is an acidic solution )


Name the following acid, and then Name the following acid, and then write the expression for Kwrite the expression for Kaa. . Assume that only one hydrogen is Assume that only one hydrogen is ionized: Hionized: H22SOSO33

[ H[ H++ ] x [ HSO ] x [ HSO33-- ] ]

[ H[ H22SOSO3 3 ]]Ka = Sulfurous

acid


Name the following acid, and then Name the following acid, and then write the expression for Kwrite the expression for Kaa. . Assume that only one hydrogen is Assume that only one hydrogen is ionized: HBrionized: HBr

[ H[ H++ ] x [ Br ] x [ Br-- ] ]

[ HBr[ HBr ]]Ka = Hydrobromic

acid


Name the following acid, and then Name the following acid, and then write the expression for Kwrite the expression for Kaa. . Assume that only one hydrogen is Assume that only one hydrogen is ionized: HNOionized: HNO33

[ H[ H++ ] x [ NO ] x [ NO33-- ] ]

[ HNO[ HNO3 3 ]]Ka = Nitric

acid


Compare and contrast the Compare and contrast the properties of acids and bases.properties of acids and bases.

( Both acids and bases are electrolytes; they cause indicators to change colors; and they react with each other to form water and a salt. Acids taste sour, bases taste bitter. Bases feel slippery. Acids react with some metals to produce hydrogen gas. )

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Chapter 12 Review- Chemical Periodicity. Chapter 12 Review - definitions electronegativity electronegativity periods periods atomic radius atomic radius