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Chemist I" Semester Exam Re e

Unit 1: Chemistry Tools

ODefine the vocabulary for the unit.

Be able to compare, contrast and identi ' examples of ea h of the following:

A Atom S{V\uv t(~JV f) t+-o CV\A.1t c«:

B. Molecule (PV'~ \€lIt Ii bOr'\dJ. G>I"'\E CMIl.~ \V'-o.de. iAf o-F\:y\.-f\e I'\V'- ~ (M,,- ",,-t-. {(\ (~i~ ,....-<.- f""-~ oe: e-k "'0+ -Ind)

C. Element <)lI\bS'.J..c~C( ~.<- ().p of-bJ\Ly one. -1y~€.O+-~'i"\ I

D.Mixture J'A:'.t4r ~t-;3 iY'~')CeJl' ~ Cf../\ 612- S-ef't~W'V/I'·~GV'.tGhe fV\tLo\'\ Ch.~~e) j

E. Compound S'u..bS/""I\.c.c.- Co fV\ p lei of- /'l (jr-£..- ·Rc.t1 OI\L ele.--melltw~.rc<~ &I\.(\ot b... .\e.r~W \...n-Ko~+ C"elV\-(c"~ dtctl\id

o Accurately use measuring equipment and scales in lab. ( ..JS J3",y,n)Review your Reading Scales worksheet and be able to perform similar

measurements.Record the correct volume measurements for each cylinder below.

1---~-1001--L-----20

f-----·40

1-----10

a) 3'1-. LmL b)~

o Perform metric-metric conversions.

1-----10

c)

1--------'-'0

Know the order of the six main prefixes and be able to use them!

Kilo Hecto Deka Base Deci Centi Milli

Perform the following metric conversions.a) 98 g = C{~,()t) Orng d) 2.3 kL = "1;301) L

;;

b) 2,34 m = '7-,!>':L ern e) 325 cL = ~'2S0 mL

/'

-,d) 0.578 5..T~ )< 10

c:; Convert between scientific no - n and regular no tion.

Write the following numbe - scientific notatio .

a) 657,000 6. Si- 'f. (

b) 0.00098 q to g X I -1-\

Write the following numbers in regular notation.

a) 4.36 x 10-7 0..0 t) 0.0.0 L{ 3.b

b) 3. 17 x 102 ~ \ "1-

e) 31,000,000 ::r'3~\ X lo

d) 6.656 x 104 "",Sf, 0

e) 5.08 x 10-4 O.oo05oQIJ Determine how many significant figures a measurement contains.

a) -.60 3b) 8 00 2.

e) 0.012 Lf) 300.4 Y

o

o Identify properties as physical or chemical.

For each of the following diagrams, decide whether each represents a physical change ora chemical change. Then, explain why!

Reaction Type: P~iS;T~lGh.(A.r:j e.Reasoning: ~ li\1Y\~. C;~ bsk<e? .

Identify each of the following as physical or chemical changes.

ChefV\ tc__C\,/ Burning paper.

V~5ic",-\ Getting paper wet.

~~s;c..~\ Ripping paper.

Unit 2: Matter

o Describe the scientists and experiments that contributed to our understanding

of the atom.

SCIENTIST DALTON THOMPSON RUTHERFORD

hJ'C\c,\ ~+>~ C~~~ ~'/ (;o\c\ ~:-~ ~;-~ J-,EVIDE CEI -\t-~ ••Id~ - ~oS["\'~ ~ f'J, '~ . _?OfVI~~~ w1\5' ~

EXPERlME T ~CI.,..h~\e}/· - ~O~} AJ{eJ-~ \~ ~~fI\e(\-b hi d\. .(\.(.,-+, £'\1'1{- <.,j

I

ATO_lIC"YfODELI 0 @ilia a Pic of it ando - 'hat it means!

(s,,\.~d .k~)

Be able to describe the basic properties of protons, neutrons and electrons.

Charge Mass Location

Proton + \"MV\, n\AJe.v..5eutron f'JM"- I~I,,",'" 11u.Jtl.A.-j

Electron

o Understand the differences between atoms, ions and isotopes.

1. Know what each of the following terms mean (be able to compare and contrastl):

Ion loS¥-,.J ej ",h..S, )D ;+ f.-.ts '\ cl"'Je

Isotope: D~e.I\t- (\~'bJr~' f'le.I.NMf\.) I ~Me YlIAMbe.r of f.~r -/-l,~~IProton: PoS;.\-i"~ ~J€..- '11\ o..-h,l"I. '7:" +h~ (h,J't.l(.S I ~e.f..u-M'';l5

~ t\.&\,+ e\e.tV1d\+ fr I).Neutron: Ate.IAt-{k-\ ~r+~ tr- ct-hfV't> Z». fht. ~lAdeIAS, OI\~J4~h

A..:f-oJV'\ c tV\0l~( uf ~<L PfJtJ (Y\

Electron: f\le.j"'~Ve.. Pcu-h'6(E!. i'(\ C\.~I +1\ o.-b~l5 4n>lhJ .1-h(. O\~"" I~~ ~ C~J.:J} of.- ~j i h4v It-bo>'\Aj'. n ~ :J't7\i'C\ /105+

P\e<\rl.\r~ \1\ AfI\'tJ

Atomic Mass: 1l~ r'lvS S of~-H1\e O'ftOr/.' fk.+erfl'tnJ by f)~M ~~

;tJ~~f r {\~V\h s. S'a~ e(e~t'\t CoLI'- h..~ )e,~1Average Atomic Mass: I' Q\..-k_fYli C ~$e.5 de.pIlr'd.!~01\ f)'lJA.tnr"0~)(}~~

~. ~ve{Q.jl!. of ~t t;t.+c,•••.•..c /V'AJ5e-s~ +iflC'\{ )t1p"plt of ~,~ e(eM</,+

Atomic Number: Ih~ (\(A.N\bar o-t- ~~+v(\S ~(\.~ oJ-atVJ: ()ehrtl1I"eJ W~+e \e;v\~..\- il- 15,

o Write and interpret atomic symbols.

Complete the following table, writing complete atomic symbols where appropriate.

Atomic Atomic Number Atomic Protons eutrons ElectronsSymbol Mass

55Fe +3 2/0 55 2/0 2q 2326-3SC1-\ 17 -35 1t 18 18

'-- \:t79Br -I 3$_ 'T-~ '35 liLt '3h35

IIB+3~ It > to

~5

IS N-3 -=l-- 15 1- ~ )07

L\O( tL. LO 40 'LD 20 18c-,

'2-<>~

I08A +1 4'1- 10~ 41 10) Lib47 g2H-1 I ~ 1

,'~

I

o Understand the concept of average atomic mass.

Using the periodic table, determine the most common isotope for each of the followingelements.

Sn Fe

o Draw basic electron orbital diagrams.

Draw electron orbital' arns for each of the following species.

o

\\,

p-3

o Draw Lewis dot diagrams for atoms.

Determine the number of valence electrons for each of the following species.

C 'L\ Si 1-\N-3 ~ 0-2~

Draw the Lewis dot structures for each of the following species.

CI1-

p F

Cs Cl

[N]3 f~i.J:l-1 [S]2 Gs,J"'-~C~·'J L:~~

What is the relationship between the columns on the periodic table and the valenceelectron~at the atoms within each column possess? \.

bvU~~ \'r--.t"'e 5'rAfV\L Co\~Mf\ ~S 1k.. f~tv\( #- of' Vo\eA(L el~.£.-~I\J

Why does Oxygen only form a -2 ion?"f+-~~~ Of\~1~ «oce. el~~s to.}{\llh ovdvJ- urb;'~lf Su ,+s~lsWhat is a valance electron? +~V"'1 •

Ge{J('~,,)7 {\ -r~( C)~k e<'b~~\ot~ ~~tY\

Why do Lewis dot structures only contain the valence electrons of a species? \(he>e oo..re. ~ af\tj Ol\~ Ol \f'\~kbk .fur bO'l\c\;'1\ C;

o Be able to identify elements b family name and period. -.....JlJetermine the name of the family each of the following elements is members of.

1. W -rft.\1\ S~~ -0 f\ ,MeJ·~l5 . 5. Br 11-PI \ 0J~n 52. Ca A IlCo..ltl\~ ;;;rth f\e~ls 6. Li AI ~lj M~\53. Ga Boro(\ 7. Sn _C=-·_~_,-=-b:...:.o...::..~..:...- _

4. S O,Xyje.f\ 8. e f\f bbk &se,S

Determine the period (row) each of the following elements is a member of.

1. Te t;~ 5. Co lltiJ

2. B 'Lr0. 6. I S~Determine whether each of the following elements is a metal, non-metal or metalloid.

1. Ge J"'~~ HulA 4. Br tJOi\. ;v\Q.kl2, ca~ 5, Te jV\et'\\lo~<£3. Se -.LlJoJ' ~~h\ 6. Ag /V\q,k\t---_

o Describe the various atomic trends on the periodic table.

In each of the following sets of elements, circle the element that best fits the property

described.

1. Smallest Atomic Radius: r@ Be?

2. Largest Atomic Radius: N, F o@

3. Most Ductile: M~@r Se?

4. Lowest Electronegativity: N, Oo@

5. Lowest Ionization Energy: K, Ca or@

o Understand the meaning of the various periodic trends.

For each of the following questions, explain what is occurring at the atomic level to

cause the described trend.

Wh does atomic radius decrease as you move across a period?~ ~rcr\tJns t!,(~ .,.r(!.il ••.s v'V\I("Q e I~okft~ ~/k ~[~I\.J Gts~r I""~ 11e

r\\Ac...I~(.d .

Why does atomic radius increase as you move down a family?AJ.c\ OI\CJ~r ox:b~~' {v. ~'1-Ch ('t:l""" VJh~h ~)4) ~ "\-hfV\ {c...~e~

~Why does electronegativity increase as you move across a period? .L1

~ All e(~U\ tr \c-AA+- '" ~ 1\ urb::iJI 't.!-Ie. -tJ....,J.- e<ri- "' I"""sf rOWe

(Rw"f:J Pi1.) vvn\ ry -\-0 ~(~-kl e\~c J \J~~\( ~O\~ ..Lv- (;''1:'1r .)\,.1.1\ -\ry +~}6S~ ~~r e\~c;/ru!\5. \ f+-irI p.1J

Unit 3: Bonding11:. Be able to define as well as compare and contrast the following terms:'ff\o.i

-

Ionic Bond ChefY"-,-u..1 bbrJ..0\f~~\.-eLf ch~0 J

Cl Be able to determine bond type (PolarlNon-polar Covalent, Ionic) based on theelectronegativity difference of two atoms.

Bond Electronegativity Difference Bond type

C-H L) s- Lv 1 - 04L\ No!\-P~\t\r I f\-t- r~vl<..-~AI-S 2.~·- LS - 1.0 ~ 0\0-.•.•..-'G"",- !en-t--B-F L\f 0 .- LtO 2;0 To 1\ ,"c.-.

o Be able to name Ionic and Molecular compounds.

Name the following ionic compounds

AIPo4AliNV\;n II\(Y1 ~iJe

CU2S04 ~~eYtE~~l~-kG L'wV) DN:kr» \'VI<\-ie.

-:ero"~) Chlo~~eFeCh

Name the following molecular compounds (and know the prefixes through hexa-)

NCb J\J~+ntJ~1 c-hI6~~ P04

Y-IV\\1,e. :rdn~~~ SeCl6

P~w;rb"'~I Jrc) KtJ e~£\e (\~lJ\(Vl H~Jlo·..;k

o Be ab e to determine he formula for Ionic and Molecular compounds.

Nitrogen trichloride ;Jc\'?>Dinitrogen tetraoxide NlCA1

Dinitrogen monoxide

Determine the formula for the following ionic compounds.

Iron (III) oxide ~~ 0:3

Strontium fluoride Sf V2:

Calcium bisulfate

Magnesium acetate

Determine the formula for the following molecular compounds.

Carbon tetrabromide

02 G'-~)~O~ .\

Of"4

'"4 ~

o Be able to draw Lewis dot structures for compounds and ions.

fe~

:0-1-\)H-

-2.

'Jo Be able to determine the shape and bond angle of a given molecule.

Determine the shape for each of the molecules in questions #4,Molecule Molecule Shape

02 '~~qrH2O IS~I\.\-NF3 ~1rQM~1SiS2 ) I 1\~o..>I"

C03-2 '"T~)OAA 1 ftC\/'<VS04-2 -re~e.J~(

Unit 4: Chemical Reactions

Determine the products for each of the following reactions and balance them.

Fe + CU(NOJ)2 ~ ~ ~O:3)<. -t- C:0<'

2Fe -\-.sC<A (tJo1\ -V 2~ (N()~3 -Be",+ 302 -7 L~03B

4f," .. ,•

rite the following ord equations in symbolic form and balance the resulting equation.Also identify the type of reaction each reaction represents.

Sodium reacts with magnesium chloride to form sodium chloride and magnesium.

+ f'AjC(2 --;l>2/Vo,LI +- j\,~Reaction type S, R----'-"v __

Silver nitrate reacts with sodium chloride to form silver chloride and sodium nitrate.

Reaction type_D.7 R"

Hydrogen gas and oxygen gas combine to form water.

Reaction type ~"t4es0Butane burns in oxygen to form carbon dioxide and water.

Reaction type Lotn b..sK'o n

Co ider the following balanced equation:

For the first substance, 3Ca(N03)2, describe what each of the numbers in the formula tellyou about the substance. Be specific!

The coefficient "3": 3 \ ! Ir l IyY)o e..(", <-5/+crl(""\I<. ~ u..t'\~is

The subscript "2":

5 ()'f..7j.Qf\ f¥1.~t.uJ~J I (\ Cjl\ jJCJ~ jDf)

'1- of- --\ta J1 cJ; ~Of) 5

The subscript "3":

Unit 5: oi' tometryWhat a ~ ole-Mole ratio means. . . r J .

·the.. ,,~ynbtr c+ fV\<>l t.5 aT otv: , ..•..bffafLV2 ('+- kke j' tz.,fVV\.k 0<, Cev~~1\ (lVtVl;\\o.!, of C\.,/'lcJ"1W2r rV1-b)~.A((!

Determine the molar mass for each of the following. Round to the nearest tenth orhundredth (one or two decimal places) and include UNITS:

Water

3'2.0.5

\cg ..~

Carbon \ '2.,OJ

CH3NH3

How many moles ofC2H6 are contained in 4.93 x 1024 molecules?

Lt As Xl 0'-'-1,,,,,,L;(. I~~b. OL-i.( 0'1--3"",(.

How many moles are contained in 45.7 g of K20?

L-\ <;.1-0. \<'2-0)( - \""01 ~ c: - L0 Y er f"lole 5 k ()]-1 q Lt .~ --- .:::> 2-

A chemical reaction produces 8.46 moles of gas. What volume will this gas occupy atTP?

~. Y b M()IS /C L:2.rli L-\ Moie.

toichiometryIron reacts with hydrochloric acid as described below.

Fe(s)+ 2HCI(aq)~ FeClz(aq)+ H2(g)

c. If 2.4 moles of HCI are consumed in the reaction, how many molecules of H2 areproduced?

'2 ~4Mol

b. If23.4g oflron is added to the HCI, how many liters (at STP) of hydrogen gas will beproduced?

2"d. If 3.46 x 10 J molecules of FeCl, are produced, how many molecules of HCI reacted?

Unit 4: Solutions*Be able to identify the solute and solvent in a solution.

* Know and understand all of the vocabulary for the unit.

_ olarityWhat is the molarity of a 1.0L solution that contains 80g ofNaOH?

How many moles of AgN03 are in 306mL of a O.SMAgN03solution?, Lpo" '30K> L

(:),,) ~)C o.iot-i: =P> f"ldl ~N~How man grams of a2C03 are required to create 2.0L of a O.IM solution?

a. MgCh -QAgN03G~ /'V'v. (N0,,> }-2s: C t ( )~'\-) M.) f J >h.~ '~ s

I/f-+ LLF t445 -i--if< -}> ~ ,-p L~q,)LCI- +L~lr -t> L~ql~)

b. Pb(N03)2 +}tICI, ~ ?bo, )+LH No ( )("'Y ...."'; <-Cs ] '''I(.

?~'t.;-- l-'~ +?- + 2-u--j7 pbClw) + -vr+ "2pffl;r'b-tJ- +-- LcJ- ~ pb cJ2(s)

c. (NH4)2S0jl ~OH -t IN \\ 0H + \("_Co~) ~~ L\ ~ l~ 1.{ (~'t)

'!Va ~=t""

lorn _-et Ionic Equations:De ermine the ionic and net ionic equations for the following reactions