UNIT TEST GRADE 10 CHEMISTRY
UNIT TEST GRADE 10 CHEMISTRY NAME
VERSION DATE
TOTAL
PART A Write True/False or Select appropriate letter in multiple choice questions
___Acids are compounds that dissolve in water to produce hydrogen ions.
___According to the law of conservation of mass, mass can be created but cannot be destroyed during a chemical reaction.
___If sodium oxide is dissolved in water and phenolphthalein is added, the solution will remain colourless
___Lithium oxide is a covalent molecule
___A lot of cleaning products are classified as bases.
___A single replacement reaction occurs when an element and a compound react, producing a new element and compound.
___A covalent bond forms when atoms share electrons to become stable.
___The correct chemical formula for magnesium sulphate is Mg2SO4
___Neutralization of an acid with a base can be an example of a double displacement reaction.
___Catalyst is added to a chemical reaction in order to slow the reaction down to a controllable rate
___A solid crystal of bluestone will dissolve faster than the same mass of powdered bluestone.
___Noble gases are very stable, and other elements try to have the same electron arrangement in their outermost electron shell as noble gases do.
___Molecular compounds are able to conduct electricity when dissolved in water
___Ionic bonds form between a metal and a non-metal.
___Which one of the following is not a property of a base:
a. Turns phenolphthalein pink
b. Turns litmus paper blue
c. Reacts with metals to produce hydrogen gas
d. Reacts with acids to neutralize them
___Which of the following is not true of a rate of a reaction?
a. The rate of reaction describes how slowly a change occurs.
b. Reaction rates can be measured by how quickly the products are forming. c. If reactants are used up faster the rate is slower
d. An increase in temperature causes the rates to increase.
___When an acid reacts with a base, the following products are created:
a. water and a metal
b. a metal and a salt
c. a salt and water
d. water and a non-metal
___Which of the following does not affect the rate of reaction?
a. concentration
b. catalyst
c. texture
d. temperature
___The products of a reaction are silver chloride and sodium nitrate. What are the reactants?
a. silver nitrate, sodium chloride
b. silver nitride ,sodium chlorate
c. silver nitrate, sodium metal and chlorine
___An antacid such as TUMS
a. neutralizes acids
b. neutralizes bases
c. is a weak acid
d. will turn litmus pink
___In a chemical reaction which of the following is not necessary:
a. a direct collision between the reactant particles.
b. sufficient energy
c. a catalyst
d. breaking the bonds in reactants and forming new bonds
___Which of the following elements would not form an acidic oxide?
a. Barium
b. Sulphur
c. Bromine
d. Phosphorus
___Magnesium oxide when dissolved in water will produce:
a. Mg 2+ and H +
b. Mg 2+ and OH -
c. Mg 2+ and O 2-
d. MgO (aq)
___When an iron nail is placed in a solution of copper(II) chloride, a red residue builds up on the nail and the solution changes colour. What type of reaction is this?
a. synthesis
b. decomposition
c. single replacement
d. double replacement
___A solution of silver nitrate is added to a solution of copper(II) iodide and a white precipitate forms. What type of reaction is this?
a. synthesis
b. decomposition
c. single replacement
d. double replacement
___Litmus red turns blue in a base
___Bromothymol blue turns yellow in a base.
___Nitrogen gas and water are produced when ammonium nitrite is heated. What type of reaction is this?
a. synthesis
b. decomposition
c. single replacement
d. double replacement
___Copper(II) oxide is produced when copper reacts with oxygen by heating it in a flame. What type of reaction is this?
a. synthesis
b. decomposition
c. single replacement
d. double replacement
___Which gas when dissolved in water results in uncontaminated rain water having a pH of 5.5?
a. sulphur dioxide
b. nitrogen dioxide
c. carbon dioxide
d. carbon monoxide
___Which of the following energy sources contributes to acid rain:
a. nuclear
b. gasoline
c. wind
d. hydroelectric
___Which of the following is incorrect about catalysts?
a. They speed up the rate of reaction.
b. They increase the rate that the reactants are used up.
c. They increase the rate that the products are created.
d. They are used up in the reaction.
___Which of the following compounds is an ionic compound?
a. H2O
b. LiCl
c. CH4
d. SO3
___What is the total atom count of the compound Ca3(PO4)2?
a. 3
b. 8
c. 12
d. 13
___What is the charge of tin in SnO2?
a. 1+
b. 2+
c. 3+
d. 4+
___Valence electrons are located in the outermost electron shell of the atom.
___The period in which an element is located on the periodic table indicates the number of electrons in the valence shell.
___Tellurium has three electrons in its valence shell.
___Noble gases are very stable; other elements give up, gain, or share electrons to acquire a valence shell like those of noble gases.
___A covalent bond forms when atoms share electrons to become stable.
___An acid and a base can neutralize each other in equal amounts and concentrations
___A single displacement reaction occurs when an element and a compound react, producing a new element and compound.
___A solution with a pH of 4.0 is 1000 times stronger than a solution with a pH of 5.0.
___Potassium permanganate will dissolve faster in hot water then in cold water.
___Which of the following is not an example of a compound?
a. PbSO4 c. H2O
b. N2 d. CH4
___What is the correct chemical formula for magnesium oxide?
a. MgO
b. Mg2O
c. MgO2
d. Mg2O2
___Which of the following describes potassium?
a. Very reactive
b. A non-metal
c. Able to gain one electron
d. A gas at room temperature
___An exergonic reaction releases energy meaning that the products have less energy than the reactants.
___Melting ice would be an example of an endergonic reaction
Part B Fill in the blanks (6)
1.Al(ClO3)3 _________________________
2.MnSO4 _________________________
3.tin (IV) sulphate ___________________
4.mercury (II) chlorate ___________________
5.H2CO3 (aq) __________________________
6.HNO3 (aq) __________________________
7.iron (III) chloride _________________
8.calcium bromide __________________
9.hydrobromic acid __________________
10.hydrosulfuric acid __________________
11.barium hydroxide ___________________
12.sodium hydroxide ___________________
PART C (20)
APPLICATION
1. (2)
______AgN03 + _____Cu ( _____Cu(NO3)2 + _____ Ag
2 (2)
______ KI + _____ PbS04 ( _____K2SO4 + _____PbI2
3. (2)
NaI + Pb(NO3)2 ( NaNO3 + PbI2
4 (2)
CaI2 + AgNO3 ( Ca(NO3)2 + AgI
Write an equation for the reaction between (4)
5. calcium hydroxide reacts with hydrochloric acid. Write the balanced chemical equation.
6. Aluminum hydroxide reacts with hydrochloric acid. Write the balanced chemical equation.
7. A student had the following results….(4)
|Acid |Base |Number of drops to neutralize |pH |
| | |acid | |
|HCl |NaOH |100 | |
|HCl |NaOH |1 | |
|HCl |NaOH |10 | |
A. However they forgot to record the pH values. They later found out that the acid solutions had pH’s of 3,4, and 5. Fill in the expected pH values for the students in the table above. (Explain your selections)
B. How many times stronger is pH 2 then 6?
C. How many times weaker is pH 4 than 1?
8. In the following equation (8)
____ MgS + ____ Na ( ____ Na2S + ____ Mg
Determine the mass of all reactants and products given that 5g of magnesium is produced.
9.
____ Cl2 + ____ KBr ( ____ Br2 + ____ KCl
Determine the mass of all reactants and products given that 5 g of bromine are produced.
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