SCH3U Chemistry Exam Review

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Chemistry practice questions

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SCH3U Chemistry Exam Review


Froggy Jumps SCH3U Chemistry Exam ReviewVersion en ligne Chemistry practice questions par Mariana 1 Which option correctly describes protons? a Neutral charge, nucleus, affect isotopes b Positive charge, nucleus, determine the element c Positive charge, electron cloud, affect mass 2 What determines the atomic number of an element? a Number of electrons b Atomic mass c Number of protons 3 What was a major limitation of Dalton’s atomic model? a It did not include subatomic particles b It placed electrons in fixed orbits c It assumed atoms were mostly empty space 4 Which observation from the gold foil experiment supported the nuclear model? a All alpha particles were absorbed b Most particles passed through, some deflected sharply c All alpha particles were absorbed 5 Why is the quantum mechanical model the most accurate? a It shows electrons in fixed paths b It explains isotopes only c It describes electrons as probability regions 6 What do elements in the same group have in common? a Same number of valence electrons b Same atomic mass c Same atomic number 7 Why are valence electrons important? a They determine atomic mass b They determine bonding and reactivity c They affect isotopes 8 Why do metals tend to form cations? a They gain electrons easily b They share electrons equally c They lose electrons easily 9 Isotopes of an element differ in their: a Number of neutrons b Number of protons c Atomic number 10 Why does abundance matter when calculating average atomic mass? a All isotopes contribute equally b More common isotopes affect the average more c Only radioactive isotopes count 11 Why does atomic radius decrease across a period? a More energy levels are added b Shielding increases c Nuclear charge increases 12 What happens to ionization energy across a period? a It increases due to stronger nuclear attraction b It decreases due to shielding c It remains constant 13 Which best describes ionic bonding? a Sharing of electrons b Transfer of electrons c Temporary dipoles 14 What does VSEPR theory predict? a Bond strength b Reaction rate c Molecular shape 15 A molecule with polar bonds can be non-polar if it is: a Symmetrical b Large c Ionic 16 The reaction A + B → AB is an example of: a Decomposition b Synthesis c Combustion 17 The reaction AB → A + B is an example of: a Synthesis b Combustion c Decomposition 18 Double displacement reactions usually occur when: a A precipitate, gas, or water forms b Reactants are solids c Energy is released 19 What are the products of a combustion reaction? a CO and H₂ b CO₂ and H₂O c C and H₂O 20 Why are states of matter included in chemical equations? a To balance equations b To identify isotopes c To show physical form of substances 21 One mole contains: a 6.02 × 10²³ particles b 6.02 × 10²² particles c 1.00 × 10²³ particles 22 What is the purpose of molar mass? a To balance equations b To convert between grams and moles c To determine charge 23 What is the correct first step in stoichiometry problems? a Use mole ratio b Balance the equation c Calculate yield 24 What determines the maximum amount of product formed? a Excess reactant b Temperature c Limiting reactant 25 Percent yield is calculated using: a Actual ÷ theoretical × 100 b Theoretical ÷ actual × 100 c Moles ÷ mass × 100 26 A solution is best described as: a A heterogeneous mixture b A homogeneous mixture c A pure substance 27 What happens during dissociation? a New ions form b Electrons are transferred c Ionic compounds separate into ions 28 What is the difference between dissociation and ionization? a Dissociation separates ions; ionization forms ions b They are the same process c Ionization occurs only in solids 29 A supersaturated solution is: a Stable with maximum solute b Unstable with excess solute c Dilute 30 What does molarity measure? a Mass of solute b Volume of solvent c Moles of solute per litre of solution 31 According to kinetic molecular theory, gas particles: a Move constantly b Are stationary c Have strong attractions 32 What causes gas pressure? a Gravitational force b Particle collisions with container walls c Particle mass 33 STP conditions are: a 25°C and 100 kPa b 25°C and 101.3 kPa c 0°C and 101.3 kPa 34 Boyle’s Law shows the relationship between: a Pressure and volume b Pressure and temperature c Moles and volume 35 Why must Kelvin be used in gas law calculations? a It simplifies math b It increases pressure accuracy c It is an absolute temperature scale

SCH3U Chemistry Exam Review

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SCH3U Chemistry Exam ReviewVersion en ligne

par Mariana

Which option correctly describes protons?

What determines the atomic number of an element?

What was a major limitation of Dalton’s atomic model?

Which observation from the gold foil experiment supported the nuclear model?

Why is the quantum mechanical model the most accurate?

What do elements in the same group have in common?

Why are valence electrons important?

Why do metals tend to form cations?

Isotopes of an element differ in their:

Why does abundance matter when calculating average atomic mass?

Why does atomic radius decrease across a period?

What happens to ionization energy across a period?

Which best describes ionic bonding?

What does VSEPR theory predict?

A molecule with polar bonds can be non-polar if it is:

The reaction A + B → AB is an example of:

The reaction AB → A + B is an example of:

Double displacement reactions usually occur when:

What are the products of a combustion reaction?

Why are states of matter included in chemical equations?

One mole contains:

What is the purpose of molar mass?

What is the correct first step in stoichiometry problems?

What determines the maximum amount of product formed?

Percent yield is calculated using:

A solution is best described as:

What happens during dissociation?

What is the difference between dissociation and ionization?

A supersaturated solution is:

What does molarity measure?

According to kinetic molecular theory, gas particles:

What causes gas pressure?

STP conditions are:

Boyle’s Law shows the relationship between:

Why must Kelvin be used in gas law calculations?