Grade 9 Chemistry SNC 1W Test

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Questions and Answers

How does the arrangement of particles differ between solids, liquids, and gases?

In solids, particles are tightly packed in a fixed arrangement. In liquids, particles are closely packed but can move around. In gases, particles are widely dispersed and move randomly.

Explain the relationship between an element's position on the periodic table (group and period) and its properties.

Elements in the same group have similar chemical properties due to the same number of valence electrons. Elements in the same period have the same number of electron shells. Properties vary across a period.

How does the density equation relate mass and volume to calculate density?

Density is calculated by dividing mass by volume ($Density = \frac{Mass}{Volume}$).

Describe 3 physical properties that can be used to identify a substance.

<p>Colour, odour, and texture are physical properties that relate to appearance. Solubility is another physical property.</p>
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Explain the difference between a physical change and a chemical change, providing an example of each.

<p>A physical change alters the form of a substance but not its chemical composition (e.g., melting ice). A chemical change involves the formation of new substances (e.g., burning wood).</p>
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What are the charges of an ion, an anion, and a cation?

<p>An ion is a charged atom or molecule. An anion is a negatively charged ion. A cation is a positively charged ion.</p>
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State the four principles of the Particle Theory of Matter.

<ol> <li>All matter is made of particles. 2. There is space between particles. 3. Particles are always moving. 4. Particles are attracted to each other.</li> </ol>
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Explain how to determine the number of neutrons in an atom, given its mass number and atomic number.

<p>The number of neutrons is calculated by subtracting the atomic number from the mass number, using the formula: # of neutrons = mass number – atomic number.</p>
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Describe how metals and nonmetals differ in terms of their malleability and conductivity.

<p>Metals are malleable and good conductors of electricity. Nonmetals are nonmalleable (brittle) and poor conductors (insulators).</p>
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How is the Bohr-Rutherford diagram useful for visualizing the structure of an atom?

<p>The Bohr-Rutherford diagram shows the arrangement of electrons in electron shells around the nucleus, illustrating the atom's electronic structure.</p>
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What information can be gained from reading a chemical formula like $H_2O$?

<p>A chemical formula indicates the elements present in a compound and the ratio in which they are combined. $H_2O$ indicates two hydrogen atoms and one oxygen atom are in each molecule.</p>
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Why is knowing if a substance is combustible or reacts with acid important?

<p>Combustibility and reactivity with acid are chemical properties. This knowledge is important for safety, handling, and predicting chemical behaviour.</p>
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Explain how an atom that gains electrons is different from an atom that loses electrons.

<p>An atom that gains electrons becomes negatively charged (anion). An atom that loses electrons becomes positively charged (cation).</p>
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Describe the difference between an atom in the ground state and an atom in the excited state.

<p>An atom in the ground state has its electrons in the lowest possible energy levels. An atom in the excited state has one or more electrons in higher energy levels.</p>
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What does it mean when it is stated that 'there is nothing between particles'?

<p>This refers to the empty space that exists between the individual atoms or molecules that make up matter.</p>
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How would you test for the presence of hydrogen gas in a laboratory setting?

<p>Hydrogen gas can be tested using the 'pop' test. A burning splint will make a popping sound in the presence of hydrogen.</p>
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What is the significance of alkali metals, noble gases, and halogens being located in specific groups on the periodic table?

<p>Their group location indicates similar valence electron configurations, leading to predictable chemical behaviours: alkali metals (group 1) are very reactive, noble gases (group 18) are inert, and halogens (group 17) are highly reactive.</p>
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List 3 of the 8 physical changes.

<p>Melting, freezing, evaporation, condensation, sublimation, deposition, ionization, recombination.</p>
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List the 3 examples of chemical changes.

<p>Rusting of iron, burning of wood, and cooking an egg.</p>
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Flashcards

Physical Property

A property that can be observed or measured without changing the substance's chemical identity.

Qualitative Property

A property that can be observed or measured with the senses; descriptive but not numerical.

Quantitative Property

A property that can be measured and expressed with a numerical value.

Chemical Property

A property that describes how a substance changes into a new substance.

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Combustibility

The ability of a substance to burn.

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Density

The amount of mass per unit volume.

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Matter

Anything that has mass and takes up space.

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Physical Change

A change that alters the form or appearance of a substance but does not change it into a new substance.

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Chemical Change

A change that produces a new substance with different chemical properties.

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Particle Theory of Matter

All matter is made of tiny particles; there is space between particles; particles are constantly moving; particles move faster when heated.

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Atomic Number

The number of protons in the nucleus of an atom; identifies an element.

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Mass Number

The total number of protons and neutrons in the nucleus of an atom.

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Period

A horizontal row in the periodic table.

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Group

A vertical column in the periodic table; elements in the same group have similar chemical properties.

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Ground State

A state where electrons are in their lowest energy levels.

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Excited State

A state where electrons have absorbed energy and moved to higher energy levels.

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Ion

An atom or molecule with an electrical charge due to the loss or gain of electrons.

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Anion

A negatively charged ion; gains electrons.

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Cation

A positively charged ion; loses electrons.

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Study Notes

  • The Chemistry SNC 1W test is on Monday, March 31, 2025
  • The test includes multiple choice (15 marks), matching (10 marks), true or false (10 marks), and short answer (15 marks), for a total of 50 marks
  • A periodic table is provided for the test.

Key Definitions

  • Physical property, qualitative property, quantitative property, chemical property
  • Physical change and chemical change
  • Matter
  • Atomic number, mass number
  • Period, group
  • Excited state, ground state
  • Ion, anion, cation

Key Concepts

  • Color, odor, taste, texture, and solubility are physical properties
  • Combustibility and reaction with acid are chemical properties
  • The density equation
  • Salt, sugar, and baking soda are soluble; baking soda reacts with acid
  • The 4 principles of "The Particle Theory of Matter"
  • There is nothing between particles
  • How particles are arranged in solids, liquids, and gases
  • Metals are ductile, malleable, shiny, and conductors; nonmetals are nonductile, nonmalleable, dull, and insulators
  • All matter is made of atoms
  • Parts of the Atom from "The Structure of the Atom"
  • How to calculate the number of neutrons using the formula: # of neutrons = mass number – atomic number
  • How to draw Bohr diagrams and Bohr-Rutherford diagrams
  • How to read a chemical formula; H2O contains two hydrogen atoms and one oxygen atom
  • Location of the Noble Gases, Alkali Metals, and Halogens on the Periodic Table
  • An atom that gains electrons is negatively charged, and an atom that loses electrons is positively charged
  • How to determine the chemical formula and chemical name given two elements that combine
  • Tests for Hydrogen, Oxygen, and Carbon Dioxide
  • List the 8 physical changes
  • List the 3 examples of chemical changes

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