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Chemistry in Action

Exercise Book

Periodic Table Scavenger HuntAnswer each question in the space provided. Refer to you Periodic Table.

1. How many periods does the periodic table have?________________________2. How many groups does the periodic table have? ________________________3. Why are the groups important in the periodic table?

______________________________________________________________________________________________________________________

4. What is special about the group of noble gases? ______________________________________________________________________________________________________________________

5. Where are the metals found in the periodic table? _____________________6. Where are the non-metals found in the periodic table? __________________7. Which elements are found around the “staircase” of the periodic table?

___________________________________________________________8. Why are these elements at the “staircase” special?

_________________________________________________________________________________________________________________________________________________________________________________

9. Which metal is a liquid at room temperature? _________________________10. What does the atomic number represent?

______________________________________________________________________________________________________________________

11. What does the atomic mass represent? ______________________________________________________________________________________________________________________

Periodic Table of Elements1. a.) Write the symbols for the first 20

elements in the periodic table below. You may use your Periodic Table.

c.) Using an orange pencil crayon, shade the elements that belong to the group of alkaline earth metals.

b.) Using a yellow pencil crayon, shade the elements that belong to the group (family) of alkali metals.

d.) Using a light green pencil crayon, shade the elements that are part of the halogen group.

e.) Using a light blue pencil crayon, shade the elements that are part of the noble gas group.

2. Why are the groups important in the periodic table?

3. What is special about the group of noble gases?

4. Describe two patterns in the periodic table.

5. Describe what happens to the elements in a group as you move vertically down the periodic table (as you go, for example, from an alkali metal in Period 1 to an alkali metal in Period 2).

Electron Dot DiagramsPractice drawing electron dot diagrams for different elements.

Element Name Symbol Family Electron Dot

Diagram

sodium

Ne

fluorine

Element Name Symbol Family Electron Dot

Diagram

Ca

magnesium

K

oxygen

Electron ShellsPractice drawing electron dot diagrams for different elements.

Element Element Symbol

Atomic Number

Number of Protons

Number of Electrons

Period Number

Number of Shells

Electron Dot Diagram

carbon C 6 6 6 2 2

aluminium

silicon

calcium

Element Element Symbol

Atomic Number

Number of Protons

Number of Electrons

Period Number

Number of Shells

Electron Dot Diagram

Li

B

P

Na + Cl Na+Cl-

Ionic BondingIonic bonding occurs when a metal transfers one or more electrons to a non-metal in an effort to attain a stable octet of electrons. For example, the transfer of an electron from sodium to chlorine can depicted by a Lewis dot diagram.

Show the transfer of electrons in the following combinations.1. K + F 2. Al + Br

3. Mg + I 4. Ca + Cl

5. Be + S 6. Al + O

7. Na + O 8. Li + O

9. Na + F 10.Mg + O

11.Ca + F 12.Be + N

13.K + Cl 14.Sr + S

15.Al + S

Covalent BondingA covalent bond is a form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms. There can be single, double and triple bonds within a molecule.

Show the sharing of electrons in the following combinations.1. C + Cl 2. S + O

3. N + O 4. H + I

5. F + S 6. P + Br

7. H + Cl 8. C + S

9. C + O 10. C + Br

11. H + N 12. N + N

13. N + F 14. P + S

15. Cl + Cl

Cross-Over MethodWrite the formulas of the compounds produced from the listed ions.

Cl- N3- O2- F- P3- S2-

Na+

Li+

K+

Ca2+

Mg2+

Zn2+

Fe3+

Al3+

Co3+

Fe2+

H+

Naming Ionic Compounds1. Name the following ionic compounds:

a. NaBr

b. Zn3P2

c. KI

d. Mg3P2

e. NaF

f. GaAs

g. ZnS

h. K3N

i. AlP

j. MgCl2

k. Be3P2

l. CsF

m. MgO

n. K2O

o. CaS

p. MgI2

q.2. Write the formulas for the following ionic compounds:

a. calcium bromide

b. gallium chloride

c. sodium hydride

d. lithium iodide

e. silver bromide

f. beryllium chloride

g. silver oxide

h. potassium sulphide

i. sodium fluoride

j. calcium nitride

k. magnesium phosphide

l. barium bromide

m. magnesium bromide

n. aluminum iodide

o. potassium chloride

p. silver chloride _________________________________

Cross-Over MethodPolyatomic Ions

Write the formulas of the compounds produced from the listed ions.

MnO4- CO3

2- OH- SO42- PO4

3- NO3-

Na+

NH4

+

K+

Ca2+

Mg2+

Zn2+

Fe3+

Al3+

Co3+

Fe2+

H+

Naming Polyatomic Compounds1. Name the following polyatomic compounds:

a. Be(HCO3)2

b. Al(CN)3

c. Sc(OH)3

d. Al2(SO4)3

e. NH4F

f. CaCO3

g. Li2SO3

h. Ag3PO4

i. NaClO3

j. KMnO4

k. Sr(MnO4)2

l. Al2Se3

m. NH4Cl

n. Li2CO3

o. Na2CO3

p. Ca(OH)2

q. K3PO4

2. Write the formula for the following polyatomic compounds

a. lithium acetate

b. beryllium hydroxide

c. zinc carbonate

d. ammonium oxide

e. potassium hydroxide

f. ammonium chromate

g. ammonium sulphate

h. silver cyanide

i. strontium acetate

j. molybdenum sulphate

k. sodium carbonate

l. ammonium sulphide

m. magnesium sulphate

n. sodium phosphate

o. aluminum sulphite

p. potassium bicarbonate

Naming Multivalent Compounds1. Write the formula for the following multivalent compounds:

a. copper (II) acetate __________________

b. cobalt (III) carbonate __________________

c. iron (III) phosphide __________________

d. vanadium (V) phosphate __________________

e. manganese (II) fluoride __________________

f. nickel (III) sulfite __________________

g. copper (II) bicarbonate __________________

h. nickel (II) selenide __________________

i. manganese (IV) carbonate __________________

j. lead (IV) nitride __________________

k. tin (II) hydroxide __________________

l. chromium (II) sulfate __________________

m. copper (II) oxide __________________

n. platinum (IV) phosphate __________________

o. nickel (III) cyanide __________________

p. vanadium (III) phosphate __________________

q. cobalt (III) sulfide __________________

r. iron (II) sulfite __________________

2. Name the following multivalent compounds

a. Cu2S

b. Mn(NO3)2

c. FePO4

d. CoCO3

e. CuSO3

f. Pb(NO2)2

g. CoSe

h. Cu(HCO3)2

i. FeO

j. Pb(SO3)2

k. CuCl2

l. V2Se3

m. Mn3N4

n. Cr(CN)3

o. SnSO3

p. VF5

q. Fe3N2

Naming Covalent (Molecular) Compounds

1. Write the formulas for the following compounds in the space provided.

a. carbon dioxide b. nitrogen monoxide

c. silicon dioxide d. tetraphosphorus decoxide e. water f. silicon carbide g. carbon disulfide h. ammonia i. diphosphorus pentabromide j. carbon tetrachloride k. arsenic tribromide l. methane m. carbon monoxide n. sulfur dioxide o. fluorine p. neon q. diphosphorus trioxide r. dinitrogen tetroxide

2. Write the names for the following compounds, in the space provided.

a. CBr4

b. N2O

c. I2

d. PF3

e. N2O4

f. Ar

g. CO

h. P4

i. NH3

j. ClO2

k. H2O2

l. SiCl2

m. SCl6

n. BH3

o. SO3

p. C2S4

q. P4O6

r. F2

Balancing Chemical Equations

1. _____ H2 + _____ O2 _____ H2O

2. _____ N2 +_____ H2 _____ NH3

3. _____ S8 + _____ O2 _____ SO3

4. _____ N2 + _____ O2 _____ N2O

5. _____ HgO _____ Hg + _____ O2

6. _____ CO2 + _____ H2O _____ C6H12O6 + _____ O2

7. _____ Zn + _____ HCl _____ ZnCl2 + _____ H2

8. _____ SiCl4 + _____ H2O _____ H4SiO4 + _____ HCl

9. _____ K + _____ Br2 _____ KBr

10. _____ Al + _____ FeO _____ Al2O3 + _____ Fe

11. _____ Fe2O3 + _____ H2 _____ Fe + _____ H2O

12. _____ P4 + _____ O2 _____ P2O5

13. _____ Na + _____ H2O _____ NaOH + _____ H2

14. _____ H3PO4 _____ H4P2O7 + _____ H2O

15. _____ C10H16 + _____ Cl2 _____ C + _____ HCl

16. _____ CO2 + _____ NH3 _____ CO(NH2)2 + _____ H2O

17. _____ Al(OH)3 + _____ H2SO4 _____ Al2(SO4)3 + _____ H2O

18. _____ Fe + _____ O2 _____ Fe2O3

19. _____ Fe2(SO4)3 + _____ KOH _____ K2SO4 + _____ Fe(OH)3

20. _____ C7H6O2 + _____ O2 _____ CO2 + _____ H2O

21. _____ H2SO4 + _____ HI _____ H2S + _____ I2 + _____ H2O

Chemical Word EquationsWrite a balanced chemical equation, including the states of matter, for each of the word equations below. 1. Aqueous sodium chloride reacts with aqueous lead (II) nitrate to yield a

lead (II) chloride precipitate (solid) and aqueous sodium nitrate.

2. Aqueous barium nitrate reacts with sulfuric acid [H2SO4(aq)] to yield a barium sulfate precipitate and nitric acid [HNO3(aq)].

3. Silver nitrate reacts in solution (aqueous) with potassium chromate to yield a silver chromate precipitate and aqueous potassium nitrate.

4. Solid calcium carbonate reacts with hydrochloric acid [HCl(aq)] to yield aqueous calcium chloride, carbon dioxide gas, and water.

5. Aqueous zinc chloride reacts with dihydrogen monosulfide gas to yield a zinc sulfide precipitate and hydrochloric acid.

6. Magnesium nitrate reacts in solution with potassium hydroxide to yield a magnesium hydroxide precipitate and soluble (aqueous) potassium nitrate.

7. Solid aluminum hydroxide reacts with nitric acid to yield soluble aluminum nitrate and water.

8. Aqueous lead (IV) nitrate reacts with aqueous sodium sulfate to yield a lead (IV) sulfate precipitate and soluble sodium nitrate.

9. Aqueous sodium hydroxide reacts with carbon dioxide gas to yield soluble sodium carbonate and water.

10. Solid magnesium oxide reacts with hydrochloric acid to yield a solution of magnesium chloride and water.

11. Solid zinc metal reacts with sulfuric acid to yield aqueous zinc sulfate and hydrogen gas

12. Solid ferric oxide reacts with solid aluminum metal to yield solid aluminum oxide and solid iron metal

Endothermic and ExothermicRewrite each word equation as a balanced chemical equation. State whether the reaction is exothermic or endothermic.1. potassium + fluorine gas potassium fluoride + thermal energy

Chemical equation: _________________________________________________________Type of reaction: __________________________________________________________

2. thermal energy + iron(II) oxide iron + oxygen gasChemical equation: _________________________________________________________Type of reaction: __________________________________________________________

3. tin + bromine gas tin(II) bromide + heatChemical equation: _________________________________________________________Type of reaction: __________________________________________________________

4. water + dinitrogen pentoxide nitric acid + energyChemical equation: _________________________________________________________Type of reaction: __________________________________________________________

5. sulfurous acid + energy sulfur dioxide + waterChemical equation: _________________________________________________________Type of reaction: __________________________________________________________

6. sodium + water sodium hydroxide + hydrogen + thermal energyChemical equation: _________________________________________________________Type of reaction: __________________________________________________________

7. calcium carbonate + heat calcium + carbon dioxide + oxygenChemical equation: _________________________________________________________Type of reaction: __________________________________________________________

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