SAINT VIATOR HIGH SCHOOL CHEMISTRY 722 MRS. COYLE

Transcription

1 STUDY GUIDE FOR SEMESTER 1 EXAM Material to know Safety in the Lab Rules Review those safety rules. Chapter 2 SAINT VIATOR HIGH SCHOOL CHEMISTRY 722 MRS. COYLE 1. What is matter? 2. What are the three states of matter? 3. Describe each one of the states of matter 4. Know what is a pure substance 5. What are physical and chemical properties? 6. Make sure that you know what are the characteristics (signs) that it is either physical or a chemical property 7. What is a mixture? 8. What is a heterogeneous and homogeneous mixtures Chapter 3 1.Scientific Notation 2. Significant figures: rules and the operations with significant figures 3. Quantitative measurement 4. Accuracy 5. Precision 6. Dimensional analysis 7. Temperature scales: Celcius to Kelvin and Kelvin to Celcius Chapter 4 1. What is the smallest part of an element that still has all the properties of that element? 2. Role of Democritus with the atom 3. Dalton s atomic theory- know the four postulates 4. Particles of an atom and its charge 5. Know how to calculate protons, electrons, and neutrons 6. Atomic number 7. Mass number 8. Isotopes

2 Chapter 5 1. Metals, non-metals, and metalloids 2. Location of metals, non-metals and metalloids in the periodic table 3. Name of vertical columns and horizontal rows 4. Know what are the majority of the elements classified as: metals, non- metals or metalloids 5. How is the modern periodic table arranged 6. Know which subatomic particle is the most important in determining how elements will react with each other? Chapter 7 and 9 1. Why type of ions do metals become? 2. Know the endings of monoatomic and polyatomic ions 3. What is the electrical charge of a cation and an anion? 4. How do ions form? 5. Name compounds are made of anions and cations 6. Which compounds are made of a non- metal combining with a non metal? II. Practice Problems Express each of the following numbers in scientific notation. a. 230 b c d. 56 million e. 2/10 f g h i

3 1. Perform the following operations and express the answers in scientific notation. a. (1.2 x 10 5 ) + (5.35 x 10 6 ) (1.2 x 10 5 ) + (5.35X 10 6 ) b. (6.91 x 10 2 ) + (2.4 x 10 3 ) c. (9.70 x 10 6 ) x (8.3 x 10 5 ) (9.70 x 10 6 ) x(8.3 x 10 5 ) d. (3.67 x 10 2 ) ( ) Signficant Figures How many significant figures do the following numbers have? 1) ) ) 890 4) ) ) ) ) 3.4 x ) 9.0 x ) x ) ) ) ) 1000

4 15) ) ) ) ) x ) 72 Solve the following mathematical problems such that the answers have the correct number of significant figures: 1) grams grams = 2) 34.1 grams grams = 3) 2.11 meters 34 meters = 4) meters 0.11 m = 5) 349 cm cm cm =

5 6) 450 meters 114 meters= 7) kilograms kilograms = 8) 84 s x s = 1. List the three states of matter and describe their basic properties: 2) Classify the following as either elements, compounds, homogeneous mixtures (solutions) or heterogeneous mixtures: a) copper (II) sulfate b) Kool Aid c) wood

6 d) plastic e) lined paper 3) Why are homogeneous mixtures more difficult to separate than heterogeneous mixtures? 4) Why can t elements be separated into smaller parts using chemical means?

7 Protons, Neutrons, and Electrons Practice Worksheet Fill in the blanks in the following worksheet. Please keep in mind that the isotope represented by each space may NOT be the most common isotope or the one closest in atomic mass to the value on the periodic table. Atomic symbol Atomic number Protons Neutrons Electrons Atomic mass B Pb Mo No 261 Yb Which group of the periodic table is most likely described by questions 1-5? 1) These elements have a charge of +2 when forming ionic compounds.

8 2) These elements are almost entirely unreactive. 3) These elements are found in group 1 of the periodic table. For problems 12-15, determine the number of valence electrons each element has: 4) sulfur 6) helium 5) carbon 7) hydrogen Electron Configuration In the space below, write the unabbreviated electron configurations of the following elements: 1) sodium 2) iron 3) bromine 4) barium 5) neptunium

9 In the space below, write the abbreviated electron configurations of the following elements: 6) cobalt 7) silver 8) tellurium 9) radium 10) lawrencium Determine what elements are denoted by the following electron configurations: 11) 1s 2 2s 2 2p 6 3s 2 3p 4 12) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 13) [Kr] 5s 2 4d 10 5p 3 14) [Xe] 6s 2 4f 14 5d 6 15) [Rn] 7s 2 5f 11

10 Determine which of the following electron configurations are not valid: 16) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 10 4p 5 17) 1s 2 2s 2 2p 6 3s 3 3d 5 18) [Ra] 7s 2 5f 8 19) [Kr] 5s 2 4d 10 5p 5 20) [Kr] Name the following ionic compounds: 1) NH 4 Cl 2) Fe(NO 3 ) 3 3) TiBr 3 4) Cu 3 P 5) SnSe 2 6) GaAs 7) Pb(SO 4 ) 2 8) Be(HCO 3 ) 2 9) Mn 2 (SO 3 ) 3 Write the formulas for the following compounds: 11) chromium (VI) phosphate 12) vanadium (IV) carbonate 13) tin (II) nitrite 14) cobalt (III) oxide

11 15) titanium (II) acetate 16) vanadium (V) sulfide 17) chromium (III) hydroxide 18) lithium iodide 19) lead (II) nitride Write the names of the following chemical compounds: 1) BBr 3 2) CaSO 4 3) C 2 Br 6 4) Cr(CO 3 ) 3 5) Ag 3 P 6) IO 2 7) VO 2 8) PbS 9) CH 4

12 10) N 2 O 3 Write the formulas of the following chemical compounds: 11) tetraphosphorus triselenide 12) potassium acetate 13) iron (II) phosphide 14) disilicon hexabromide 15) titanium (IV) nitrate 16) diselenium diiodide 17) copper (I) phosphate 18) gallium oxide 19) tetrasulfur dinitride 20) phosphorus

13 Name the following acids and bases: 1) NaOH 2) H 2 SO 3 3) H 2 S 4) H 3 PO 4 5) NH 3 6) HCN 7) Ca(OH) 2 8) Fe(OH) 3 9) H 3 P Write the formulas of the following acids and bases: 10) hydrofluoric acid

14 11) hydroselenic acid 12) carbonic acid 13) lithium hydroxide 14) nitrous acid 15) cobalt (II) hydroxide 16) sulfuric acid 17) beryllium hydroxide 18) hydrobromic acid

15

16

17

18