Teacher Period. Academic Chemistry 2015 Fall Final Exam Review due the DAY YOU TAKE THE FINAL FOR 5 BONUS POINTS on t e final exam

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1 Name Ke Teacher Period Complete the chart. Academic Chemistry 2015 Fall Final Exam Review due the DAY YOU TAKE THE FINAL FOR 5 BONUS POINTS on t e final exam Un t 1 - Matter and Chan e Definite shape? (v/n) Definite, volume? (v/n) Effec of Pressure? Density (hlqh/med/low) Solid V kjoaj Liquid l\j k)@ajls j\6ix Gas N es 2. What is a physical property? 3. What is a chemical property? ML f ': c gci _ I 4. Write (I) for intensive and (E) for extensive property: mass.!z7 density melting point -M- length conductivity IX color texture X ductility E luster volume 5. What is a physical change? 6. 7, What is a chemical change? t». List the 4 indicators that a chemical change has occurred_ 6k, ':Pra \'p~')'( c l&. 8. Classify the following as physical (P) or chemical (C) changes: food spoils candle melts - salt dissolves In water 'P burning coal C. 9. What Is the law of conserva ion of matter (or mass? L f\j ('W!:/ U AL Tf/lc cqta lo PAc According to t e law of conservation of matter, if grams of sodium are added to grams of chlorine, how much sodium chloride should be produced? M Cj 7zR as-i 3S.i G J acf 1 I a' - 1 / f ) 2 S 11, Calculate the density of a substance with a mass of 6.25 g that occupies a volume/of 5,2 mjl.! h2-6 ±. V 72 W1- /vc. 12, Gold has a density of 19.3 g/ml. Calculate the mass of a piece of gold that occupies 7 ml. Y

2 13. Classify each substance as element, compound, or mixture. zinc salt copper_ S iver C )river water, i xygen kool-aid 14. Classify each mixture as homogeneous or heterogeneous Sugar water. RM iced tea t M&M s oreo cookie_ frt A soda sugar. water_ soil Gatorade M PrT Unit 2 - Safety and Scientific Measurement 1. What is I > the proper LI 1C attire Qi-UliC for lab activities I I \IAU (5 things)? V M-l -* ry y.. q les cipw J&scty to s ge If an accident or spill occurs, you should al ays Q l. ) /hat is the proper procedure when heating materials in lab (3 things)?» & I. ih )va> er fe' iim Jf i fa'k<x *V NtAJtr 4. To dispose of all chemicals you should I )\ a f ' 4 : rcfe 5. How many significant figures are in the following numbers? a > b c. 875,000 r C ' d f Complete these problems using correct sig figs in answer, a m x m (9-0 3 b. 302,000 mm x 3.5 mm = [( m 1 c s s = d. 765 g g = <S ) g:: 3.2 m s = 0 0 /$ I

3 V nt k ClhA'\.L0nP. 9. Three different students measured a 26.30em length of twine three times each. Indicate if the student was accurate, precise, BOTH, or NEITHER! Trial 1 Trial 2 Trial 3 Accurate, Precise, Both, Neither Rachel cm cm cm hojt l A f reaie Chloe cm cm cm hi " Roel cm cm cm P ea&o, A < Unit #3 - Atomic Structure I / /] /) f / 1. What is an Atom? John Dalton 2. All matter is made up of. <f>,e0l%mjlw( particles called 3, Atoms of one element are the A(V\? Atoms of different elements are Ernest Rutherford 4. Discovered the nucleus in the gold foil experiment. Most alpha particles passed through unaffected = > concluded the atom is mostly space. Few particles deflected greatly =>concluded r e. that at the center of the atom was a small, nucleus with a charge. J. Thomson 5. Discovered the. in his investigations with a Crookes tube. Found ALL substances contained these charged particles. Stated the atom must be a dump of -p g 'De doped the charged material with negatively charged particles dispersed throughout. model of the atom based on how he theorized 7. Define atomic number - mass number average atomic mass -. Isotope,5 A moved around the nucleus. jd- ft eioft S o c ht'o feti*' dujzml9 PA V /sbio WP i 8. The nucleus of an atom is composed of. Vr( and

4 9. Isotopes have the same number of but different numbers of 10. Are the me following r groups of atoms isotopes? (YES or NO) a K) b. 8 protons and 9 neutrons 8 protons and 8 neutrons 5 protons and 6 neutrons 6 protons and 6 neutrons c.. L* I7 e Sr,Sr Si-15 and P p+ and 30 n 25 p+ and 33 n 11. Most of the? of an atom is in the mucffo LARGER SMALLER ) mass than electrons. 12. Why are'afoms neutral (no charge)? P because protons and neutrons have a 13. Nitrogen has two naturally occurring isotopes, nltrogen-14 and nitrogen-15. The atomic mass of nitrogen Is amu. Which isotope is more abundant in nature? H. 14. What is the charge on a roton a neutron P..., and an electron _!? 15. what is the mass, in amu, of a proton I, a neutron!_, and an electron &? 16. What does the number 60 in cobalt-60 mean??. - 1 /. H ic\. C I 1C I ML/VVi y Symbol Atomic # # of protons # of neut ons # of electrons : Mass # (D 8 8!6> i k> 7 14 T llna II a 12, II Lj I.O Calculate the atomic mass of the following element with the given isotope information i. : tofftr,amu 1S?Ag= 52.34% Ag= 47.66% /2>f 01 'i ' b 19. Write the shorthand nptatidn for a particle which has 9 neutrons and 10 protons. If u , Write the shorthand notation for a particle with a mass # of 88 and 38 protons. Lead-206 has _ neutrons. How many particles are in the nucleus of this radium atom? 22slRci An alpha particle is the same as the nucleus of a atom. It has a m,. W. charge. 24, A beta part cle is a high-s eed la. and has a I charge. It is the product of a becoming a _ f-o ]

5 25, Balance the following nuclear reactions: a,? -Se + b, 1 O He + 2gfPb 4 C. 4 d. 2 Pu fhe -ie + 1soSn, + <» 26, For the following decay prompts, write the complete nuclear reaction, a, Bohrium-272 decays by alpha em ssj n lo 10 b. The decay of rhodium by beta emission { 27. Complete the chart: Type of Radiation Beta Shorthand Notation O. Materia! needed to stop/shield ra iation Alpha hp A Cf Gamma " How far does radiation penetrate a person?. S m O on / QJd fliemil( Unit #4 - Waves and Electrons //) 1. What is the frequency of a wave if its wavelength is 5.25 x m? 1 ' c_ 3,d /qvpmjs _ >00 2. What is the energy of light having a frequency of 5,00 x 1012 Hz? * -f f 7 = ' -f - /s saa r 3. What is the energy of a wave If its wavelength is 7.70 x 1016 m? K( 0 j h.x= 'h- = (e&xcpt'tf-s < 1 5 4, What s the difference between an excited and a ground state electron? > fe elgj.lr/-en i h 4 gjaf/4 5. Valence Electrons - Electrons In the gained or Lost 6. A(n) ( hv i QO bm&i nergy level of Atom. This is where electrons can be has a high probability (90%) of containing an electron. fv IA. 7. What element has the Identifying square 4p3? 8. The atomic number for an element with an electron configuration of Is 22s 22p 63s2 Is?

6 9. Write the complete electron configuration for the following elements. a. sodium b. silver?ebi4 5S hp si 3 c. krypton 10. Write the noble gas configuration for a. manganese. $ Ar tfs. b. bromine. Sis' dr ' 11. Write the orbital notation for Mo (Molybdenum). enum). ll i- L l1- IV! IV 1* 1L ItltlV i zs "ep Jf 3 p Hi r 12. Complete the chart about sublevels and their orbitals. s p d r Shape mb U < \<?\)Or # of orbitals 1 T. Maximum # t., l </ of e- Major Categories of Elements Unit #8 Periodic Table 1. Groups on the periodic table are/ VERTICAL COLUMPIS / HORIZONTAL ROWS,). 2. Elements in a GROUP havesimilarcrefnical and physical have the same number of. 3. List all Elements with Similar in physical and Chemical Characteristics as Calcium: \e& _. This is because they c(. 4. PERIODS on the periodic table are ( VERTICAL COLUMNS HORIZONTAL ROV S ). Elements in a period have the same number of OhQ M lu UOtS Elements in a period have K) property similarjty. side of the periodic table. Metalloids are found along the., SY 6. Write the symbols for all of the metalloids:.line (except i 1_>. - b.i P. 5, Metals are on the side of the periodic table (except i ). Nonmetals are on the Classifying Elements 7. Octet Rule-Atoms want. 8. Groups 3-12 are called esowr ekn&i their Outer Energy Level 6

7 9, Complete the following chart 1 i I 2 13 ' ; ame Of Group MWi? NA NA NA NA Valence Electrons I 2 3Eaj i L/ r 6 r si, Gain or Lose Electrons. lose tee O idation # ** - 3 Periodic Trends / k T i (t i -i. - o A I klo JL 10. Draw and label arrows in the periodic tables that represent the 4 trends discussed in class, You must write,the name of the trend in the box below the periodic table. - JK Element Identification a. The smallest noble gas atom. f. Alkaline earth metal in Period 6, g. Metalloid in Period 2, b. 3 valence electrons in Period 4. B O S c. The element in period 2 with 7 valence e-. h. Nonmetal in Group 14, d. Halogen in Period Element in period 3 that forms a +2 ion. *~ 7 e. The most reactive alkali metal. j. Element in period 5 that forms a -1 ion. Trend Application,e\ 1, Which of the following is most electronegative? Li, B, N or Ne 2, Which of the follow ng is most reactive? ( Rb, Nb, or Ag 3, Which of the following is least reactive? 0, S, Se, o Po 4, Which of the following has the largest atomic radius JJ B, Ne, or F 5, Which of the following has the greatest ionization energy? C, S, Ge or Pb 7

8 Unit #6 -Naming 1, Nonmetals either have,, or valence electrons, t GAIN ) LOSE ) electrons to form ( + Vcharged ions called ( CATIONS / NIONs)). 2. Metals either have _],, or S valence electrons, ( GAIN /( LOSE electrons to form i +) / ~ ) charged Ions called 3. What is the Octet Ryle? l s n \ M \ S / ANIONS ). r 7 J '1 c ' mu (tti i 4. List the 10 prefixes used for naming covalent c )mpo jnds: I W\0W> 5. Complete the chart, cq < -j-pi 4? Mn I Chemical 1 Formula Covalent (C), Ionic (I), Polyatomic Ionic (P), Ionic with Transition Metal (T), Acid (A) NaNOs s 1 SII4 V j o (/X T) Chemical Name [/i N2O3 - LisN AIPO4 N1F2 ' ' ; r p : L1A11X ' kqsl H3PO4 BaS nt ::r 3 J X 4 r f\ t Ml XI 5 I iczzj NH4Br Xf i {N\MQ(/\\ 4k5 Jit 43 HCI b l/\ A fi0c \. lo pig ft Ac ) \WAJ -2* FeS04 I ' rp P2O5 )\pl phtooe pcu -0)i A t? CoClS + 5 :j:t Cd h c\ { D( fe 8

9 10. Complete the chart. Chemical Name dichlorine heptoxide iron (II) cyanide Covalent (C), Ionic (I), Polyatomic Ionic (P), Ionic with Transition Metal (T), Acid (A) c xtp Chemical Formula calcium nitride cjpm gold (I) sulfide T AxS trisillcon tetranitride (L phosphorous acid p i Hi PT sulfur hexachloride x"1 * x.. ST, magnesium phosphor de sodium oxide barium acetate X J-l p tetraphosphorus decoxide c Py Oi calcium hydroxide? CaLo nitric acid A,;. t-wo; 9

10 1. What is a mole?. 2. What is molar mass? 3. What are the 3 types of representative particles? Unit #7 - Moles.dl'tfn i> ti ks s &( <x,. Iholotvi, f / Ml/k Use the conversion guide: MASS (g) MOLES - PARTICLES i mol molar mass(g) if), ft 4, Calculate the molar mass of Ca3(P04)2. i, 6.02 x 1023 particles 1 mol $ t 5, How any moles are in 3.54 grams HhS?.l&'iM / 6. How many grams are In l.y? moles of carbon dio ide? izjdlt +* LfLl.Ol j jim ( 7. How many atoms are in 700 g of lithium? a$i tvr j '! y> k L I MD I 8. How many molecules are <9,42 wujl ;A n 0.42 moles of shs? tf' 9. Calculate the % composition for Barium in Ba(OH)2. "B-4 y. 0 1 a i 9 H f? / //C 4 A I / WT 80 3\ 18- l\ \M = 10

Academic Chemistry 2016 Fall Final Exam Review DUE THE DAY YOU TAKE THE FINAL FOR 5 BONUS POINTS on the final exam

Name Teacher Period Academic Chemistry 2016 Fall Final Exam Review DUE THE DAY YOU TAKE THE FINAL FOR 5 BONUS POINTS on the final exam Unit 1 Matter and Change 1. Complete the chart. Definite shape? (y/n)