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By: Mrs. Raghad, Chemistry teacher

Final Exam Revision Sheet

Term-3 Chemistry

Grade (10)

2018 / 2019

Name: ………….……………………

Grade: 10 ( A – B – C )

Date : ……………………..…………

The Material included in the Exam.

You should Study from:

1- Textbook: Chapter (7) Lesson (1) , (2)

2- Interactive Book: Pages (213 - 229)

3- Chapter (7) Lesson (3)

4- Interactive Book: Pages (230 - 237)

5- Chapter (8) Lesson (1)

6- Interactive Book: Pages (253 - 260)

7- Revision sheet, Quizzes

8- The worksheets given and Homework sheets

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By: Mrs. Raghad, Chemistry teacher

NGSS: HS – PS1. B.3

PART A : OXIDATION NUMBERS:

A) Define the oxidation number? P. 225-226

....................................................................................................................

………………………………………………………………………...….

B) Write the SUM of the oxidation state on the atoms in the following:

a) H2 SO4 …………

b) SO4 -2 …………

c) Br2 …………

d) He …………

e) CO3 -2 …..……

f) NO2 - …………

1. What useful functions do oxidation numbers serve? P.225

1. ………………………………………………….…

2. ……..…….………………………………………..

3. ……………………………………………….……

2. Assign the Oxidation numbers to “each atom” in these compounds: p.227

a) K Cl O3 …………… ……..……… ……………….

b) Cl O2 …………… ………..…… ……………….

c) P2 O5 …………… ……..……… ……………….

d) CO3 …………… ………..…… ……………….

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By: Mrs. Raghad, Chemistry teacher

3. Fill in the blanks with suitable complete, write the oxidation number for each

Rule: p.226

a) Pure elements: O2, P4, Na, Br2 the oxidation number is ……………

b) Fluorine oxidation number is …………….…

c) Oxygen oxidation number is usually ……………… but in OF2 is …………

and in H2O2 is ………….

d) Hydrogen oxidation number is …………… But when hydrogen combined

with metals the oxidation number is ………………

e) Ionic compounds: oxidation numbers equal their charge:

Na + oxidation number is …………

Ca +2 oxidation number is …………

Cl - oxidation number is ………….

4. Write formulas for the binary ionic compounds formed between the

following elements: p.229

a) Potassium and iodine ……………………………..

b) Aluminum and sulfur ……………..………………

c) Magnesium and chlorine ………….………………

d) Aluminum and nitrogen …………….…………….

e) Sodium and sulfur ………………….…………….

5. Name the binary ionic compounds indicated by the following formulas:

a) Ag Cl …………………………………..

b) Ca Cl2 ………………………………….

c) Zn O …………………………………..

d) Ba (OH) 2 ………………………………

e) Ca Br2 …………………………………..

f) Mg I2 ……………………………..……..

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By: Mrs. Raghad, Chemistry teacher

6. How many atoms are present in each of these formula units?

________________ a. Ca (HCO3)2

________________ b. C12H22O11

________________ c. Fe (ClO2)3

________________ d. Fe (ClO3)2

7. Circle the right answers : p.229

a) What is the correct formula for the compound made of Magnesium and Nitrogen?

a. Mg3 N2

b. Mg2 N3

c. Mg N2

d. Mg N

b) Oxidation numbers are used to indicate the …..

a. charge on an ion.

b. number of atoms or ions in a compound.

c. type of bond holding particles together in a compound.

d. distribution of electrons among the bonded particles in a compound.

c) Atoms have an oxidation number of zero:

a. pure element.

b. acid.

c. ionic compound.

d. molecular compound.

d) What is the oxidation number of nickel in Ni CO3?

a. 0

b. +1

c. +2

d. +3

e) What is the oxidation number of phosphorus in the 3

4PO ion?

a. 3 b. 0 c. +5 d.+8

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By: Mrs. Raghad, Chemistry teacher

PART B: Using Chemical Formulas:

1. Label each of the following statements as True or False: p.230-234

________________ a. If the formula mass of one molecule is x u, the molar

mass is x g/mol.

________________ b. Samples of equal numbers of moles of two different

chemicals must have equal masses as well.

________________ c. Samples of equal numbers of moles of two different

molecular compounds must have equal numbers of

molecules as well.

2. How many moles of each element are present in a 10.0 mol sample of

Mg(CO3)2?

…..……….. mol of Mg ……………… mol of C2 …………….. mol of O6

4. Consider a sample of 10.0 g of the gaseous hydrocarbon C3H4 to answer the

following questions:

a- Mass number of C = …………

b- Mass number of H = …………

c- Molar mass of C is ……. C atoms X ……………. = ………….. u

d- Molar mass of H is ……. H atoms X ……………. = ………….. u

e- Molar mass of C3H4 = .............+ .............. = ……………….. u

1. How many moles are present in this sample?

2. How many molecules are present in the C3H4 sample? Av. no. = 6.022x1023

3. How many carbon atoms are present in this sample?

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By: Mrs. Raghad, Chemistry teacher

:Percentage composition-FormulasChemical PART C:

a) Find the percentage composition of C3 H 8

1- Molar mass of C …………………..

2- Molar mass of H …………………..

3- Molar mass of C3 H 8 …………………..

4- Per. comp. % of C3 = ………………….. X 100%= ……….

5- Per. comp. % of H8 = ………………….. X 100%= ……….

6- Check ! ……………………

PART D: Describing Chemical reactions:

b) Complete the following equations: (p.253-260)

1) Acid + Base ……………… + ………….……

2) HCl + NaOH ……………… + ……………….

3) 2HgO ………………. + ………………

4) Na2O + H2O ………………………

5) Methane + Oxygen ..…………… + ………………

6) CH4 + 2O2 ……………..... + .……….……..

7) (NH4)2 Cr2 O7 …………… + ……………… + …………….

8) 2H2O …………… + ………………

GOOD LUCK!