Grade 10 Chemistry Unit Review To complete this sheet you will need your periodic table and list of polyatomic ions

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1 Grade 10 Chemistry Unit Review To complete this sheet you will need your periodic table and list of polyatomic ions Date: Part 1 The Structure of the Atom 1. List the three sub-atomic particles. After the name of each particle, indicate its charge in brackets. Electron ( - ) Proton ( + ) Neutron ( 0 ) 2. In the space below, draw a picture of an atom of lithium (draw the neutrons and protons). Be sure to include the correct numbers of subatomic particles and have them in the correct location. 3. Of the three subatomic particles, which has the most mass? Protons and neutrons 4. Of the three subatomic particles, which has the least mass? Electrons 5. What is the name of the outer shell of an atom? Valence shell 6. What are electrons in this shell called? Valence electrons 7. Why are these electrons more important than the others? They are the only particles involved in chemical bonding Part 2 Using the Periodic Table w 1. Identify each of the letters in the symbol below (i.e. what information goes in each letter s location?): 1

2 A x y A W X Y Element symbol Isotope number Atomic number Atomic mass 2. What are groups on the periodic table? Columns 3. Give three examples of groups (i.e. their names) Alkali metals, alkaline earth metals, halogens 4. What do all elements in a group have in common? Same number of valence electrons 5. What are periods on the periodic table? Rows 6. What do all elements in a period have in common? Same number of electron shells 7. Identify the element that is in: a. Group 1 period 4 Potassium (K) b. Group 13 period 5 Indium (In) c. Group 2 period 7 Radium (Ra) 8. Give examples of two elements that are in each of these categories. You MAY NOT use the same element twice: a. Metals Potassium Cobalt b. Non-metals: Phosphorus Oxygen c. Metalloids: Boron Silicon d. Alkali metals: Lithium Sodium Other answers are possible e. Alkaline Earth metals: Beryllium Magnesium f. Transition metals: Scandium Iron g. Halogens: Fluorine Chlorine 2

3 h. Noble gases: Helium Neon 9. Complete the table below; Element Atomic Atomic Metal, nonmetal, Valence Symbol Protons Neutrons Electrons name number mass or metalloid electrons Rubidium Rb Metal Selenium Se Non-metal Bromine Br Non-metal Calcium Ca Metal What is an isotope? A different version of an element where the number of neutrons are different. Example carbon 12, carbon 13 and carbon 14 are different isotopes of carbon. Part 3 Atoms, Ions and Bonding 1. List two differences and two similarities between Bohr and Lewis models of the atom: Bohr Lewis Differences Similarities Show all electrons Shows protons and neutrons Does not show element symbol Show valence electrons Model of the atom Show only valence electrons Does not show protons and neutrons Shows element symbol Show valence electrons Model of the atom 2. Draw a Bohr model and Lewis diagram for each of the following three elements Nitrogen Aluminium Argon 3

4 7p + 13p + 7n 0 14n 0 18p + 22n 0 Bohr model N Al Ar Lewis diagram 3. What is an ion? An atom with an unequal number of protons and electrons (a charged particle) 4. What is the difference between a cation and an anion? Cation has a positive charge, anion has a negative charge 5. Complete the table below for anions and cations Particle Name Charge More p + /e - Gain/Lose e - Type of Element (metal/non-metal) Cation + Proton Lose Metal Anion - Electrons Gain Non-metal 6. Complete the table below by indicating the ion symbol and the name of the ion for these six elements Elements Ion symbol Ion name Elements Ion symbol Ion name 4 Sodium Na + Sodium ion Phosphorous P 3- Phosphide Selenium Se 2- Selenide Aluminium Al 3+ Aluminium ion Calcium Ca 2+ Calcium ion Bromine Br - Bromide

5 7. List three differences between ionic and covalent compounds/bonds (differences in naming do not count) I: electrons are exchanged/gained and lost; C: electrons are shared I: involves metals and non-metals; C: 2 non-metals I: ions involved; C: ions not involved 8. Complete the table below by identifying whether the compound is covalent or ionic Compound Ionic or Covalent Compound Ionic or Covalent SiO 4 Covalent WS 3 Ionic SrSe Ionic Li 3 N Ionic CaI 2 Ionic C 4 H 10 Covalent 9. For transition elements: a. Where are they found on the periodic table? In the middle of the table b. What kind of elements are they? Metals c. What does the Roman numeral next to a transition element indicate? The charge of the metal 10. Complete the table below by indicating the Arabic numeral next to the roman numeral (note the numbers are NOT in order): VI 6 I 1 VII 7 III 3 VIII 8 IX 9 V 5 II 2 X 10 IV 4 5

6 11. Why do we use prefixes with covalent compounds and not with ionic compounds? Ions of two elements can combine in only one ratio so indicating the number of atoms of each element is unnecessary. Two non-metal elements can combine in multiple ratios, therefore we need to indicate the number of atoms of each element 12. Complete the table below by indicating the correct prefix for each of these numbers: 1 Mono 2 Di 3 Tri 4 Tetra 5 Penta 6 Hexa 7 Hepta/septa 8 Oct 9 Nona 10 Deca 13. For polyatomic ions: OMIT THIS QUESTIONS a. What does the name polyatomic ion mean? Ions with more than one atom b. Why do they have a charge? Because they have an unequal number of protons and electrons 14. Complete the table below by first indicating whether the compound in covalent or ionic, and then giving the correct formula or name. Name/Formula Covalent or Ionic Name/Formula a) Zinc II oxide I ZnO b) Silicon dioxide C SiO 2 c) Na 2 O I Sodium oxide d) Magnesium nitride I Mg 3 N 2 e) B 2 Br 4 C Diboron tetrabromide f) SnSe 2 I Tin IV selenide g) Manganese IV oxide I MnO 2 h) CCl 4 C Carbon tetrachloride i) V 2 S 3 I Vanadium III sulphide j) OMIT Ni(H 2 PO 4 ) I Nickel II dihydrogen phosphate k) OMIT Gold I nitrite I AuNO 2 l) B 3 H 4 C Triboron tetrahydride 6

7 m) Nitrogen nonaoxide C NO 9 n) Si 2 F 3 C Disilicon trifluoride o) OMIT Ammonium oxide I (NH 4 ) 2 O p) OF 2 C Oxygen difluoride q) OMIT W(SO 4 ) 3 I Tungsten VI sulphate r) Carbon diodide C CI 2 s) OMIT Ca 3 (PO 4 ) 2 I Calcium phosphate Part 4 Chemical Reactions 1. Complete the table below by indicating the correct number of atoms of each element: Atoms of Each Element 5NH 4 Cl N 5; H 20; Cl 5 W 2 (SO 4 ) 3 W 2; S 3; O 12 3(NH 4 )CO 3 N 3; H 12; C 3; O 9 4Al(C 2 H 3 O 2 ) 3 Al 4; C 24; H 36; O What is the law of conservation of mass? During a chemical reaction matter/mass cannot is neither created nor destroyed 3. Balance the following chemical equations: a. 1 KI + 4 F 2 1 IF KF b. 2 CuO + CuS 3 Cu + 1 SO 2 c. 8 H 3 N + 3 Br 2 6 NH 4 Br + 1 N 2 7

8 d. 3 I HNO 3 6 HIO NO + 2 H 2 O (HARD ONE) 4. Correctly write out, then balance the following equations: a. Nitrogen gas reacts with water to form hydrogen gas and trinitrogen pentaoxide 3 N H 2 O 10 H N 3 O 5 b. OMIT Ammonium phosphide reacts with table salt to form ammonium chloride and sodium phosphide 1 (NH 4 ) 3 P + 3 NaCl 3 NH 4 Cl + 1 Na 3 P c. Vanadium III oxide reacts with calcium bromide to form vanadium III bromide and calcium oxide 1 V 2 O CaBr 2 2 VBr CaO d. Methanol (CH 3 OH) burns in a combustion reaction 2 CH 3 OH + 3O 2 2 CO H 2 O 5. Identify the type of reaction in each of the following equations 8 a. CH 2 CH 2 + Br CH 3 CH 2 Br SYNTHESIS

9 b. CaCO 3 CaO + CO 2 DECOMPOSITION c. ZnF 2 + Li LiF + Zn SINGLE DISPLACEMENT d. C 3 H 8 + O 2 CO 2 + H 2 O COMBUSTION e. Ca(C 2 H 3 O 2 ) 2 + Na 2 CO 3 CaCO 3 + NaC 2 H 3 O 2 DOUBLE DISPLACEMENT 9