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Science 9 GTHS > 9B: Matter and Chemical Change > Flashcards

9B: Matter and Chemical Change Flashcards

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1
Q

WHMIS =?????????

A

Workplace

Hazardous

Material

Information

System

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2
Q

MSDS=????

What type of information would you find on them?

A

Material Safety Data Sheets

These sheets provide helpful information on how to use, store, transport, and react to chemicals if an accident were to occur.

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3
Q

Matter is ___________.

A 
Matter is anything that has mass and
occupies space(volume).
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4
Q

A state change from:

  • Solid to a liquid is ____________.
  • Liquid to a gas is ___________ (also known as vaporization).
  • Gas to a liquid is ___________.
  • Liquid to a solid is ___________.
  • Solid directly into a gas; this process is called ___________.
  • Gas directly to a solid. This is called ___________.
A

A state change from:

  • Solid to a liquid is melting.
  • Liquid to a gas is evaporation (also known as vaporization).
  • Gas to a liquid is condensation
  • Liquid to a solid is freezing
  • Solid directly into a gas; this process is called sublimation
  • Gas directly to a solid. This is called deposition
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5
Q

Can you describe four main points of the PARTICLE MODEL OF MATTER?

A

This model consists of four main points:

  1. All matter is made up of tiny particles
  2. There is space between these particles
  3. Those particles are always moving
  4. The particles may be attracted or bonded to each other.
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6
Q

Gases are more dense than liquids. True or false?

A

False, liquids are more dense than gases because their particles are closer together.

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7
Q

What is the difference between evaporation and condensation?

A

Evaporation- its when you boil a liquid and it slowly changes to a gas. Condensation- is when a gas is cooled to form a liquid

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8
Q

Properties can be described as ____________.

A

Properties are characteristics that can be used to describe a
substance.

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9
Q

Explain what a physical property is, and provide a few examples of some physical properties.

A

A physical property is a characteristic of matter that can be observed and measured without changing the chemical identity of the sample.

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10
Q

What is the difference between boiling point and melting point?

A

The melting point of a substance is the temperature at which it changes from a solid to a liquid.

The boiling point of a substance is the temperature at which its liquid phase changes to the gas
phase.

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11
Q

What is the difference between the terms ductilty and malleability?

A

Any solid that can be stretched into a long wire is said to be ductile. The most common example of a ductile material is copper.

A substance that can be pounded or rolled into sheets is said to be malleable. Metals such as gold and tin are malleable. Aluminum foil is an example of a product made from a malleable
substance.

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12
Q

Define physical change?

A

Physical change occurs when matter changes size, shape, or state. It is reversible.

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13
Q

What is the difference between a chemical property and a chemical change?

A

A chemical property describes how a substance interacts with other substances such as acids.

A chemical change always results in the formation of a different substance or substances. It is usually irreversible.

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14
Q

What are 5 examples of chemical properties of matter?

A
  • reactivity with acids
  • ability to burn
  • reaction in water
  • behaviour in air
  • reaction to heat/cold
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15
Q

How can you distinguish a pure substance from a mixture?

A

A pure substance is made of only one kind of matter and has a unique set vof properties that sets it apart from any other kind of matter.

A mixture is a combination of two or more substances that are not combined at a molecular level.

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16
Q

What is an element and how are they related to compounds?

A

An element is a material that cannot be broken down into any simpler substance.

When two or more elements combine chemically-that is, in specific, fixed proportions-they form a compound. When the elements hydrogen and oxygen are combined in specific proportions, they form the compound water.

Elements are organized into a periodic table according to their properties. Each element has its own symbol. For example, hydrogen is H, carbon is C, and oxygea is 0.

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17
Q

What is a mixture, and what are the four main types of mixtures?

A

A mixture is a combination of pure substances. However, the substances in a mixture do not combine chemically as happens when a compound is formed.

  1. Mechanical Mixture
  2. Solution
  3. Suspension
  4. Colloid
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18
Q

What is the difference between a heterogeneous and a homogeneous mixture?

A

A heterogeneous mixture is a combination of two substances where you can clearly see the different materials.

Homogeneous refers to a uniform mixture where the substances are hard to differentiate/see the difference.

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19
Q

What is a good example of a mechanical mixture and why?

A
  • Trail Mix
  • Bird Seed
  • Macaroni Salad
  • Chocolate Chip Cookies

These are good examples of a mechanical mixture because they are heterogenous and can be easily separated into different components, even by hand in some cases.

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20
Q

Distinguish between a solute and a solvent. Provide an example.

A

Solute= IS DISSOLVED

Solvent=DOES THE DISSOLVING

For example, if I were to make hot chocolate in milk, the powder acts as a solute and the milk would be the solvent since it is dissolving the powder.

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21
Q

What is a good definition of a solution? Can you think of two examples of solutions?

A

A solution is a mixture where one substance dissolves into another. For example, lemonade and iced tea are both examples of solutions. In addition, soda will have carbonation or diissolved gases in them.

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22
Q

The solvent is the substance that dissolves in the solute True or False?

A

False the solvent dissolves the solute Ex/ Water dissolved the juice powder

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23
Q

A saturated solution is a mixture where _______.

How can you tell if a solution has become saturated?

A

No more solute can be dissolved in a given volume of solvent.

  • You will often see solid solute particles settled at the bottom.
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24
Q

What is the difference between a solution and a suspension?

A

A suspension is when a substance floats on top of another substance because it can’t dissolve. A solution is a mixture which is fully dissolved into a solvent.

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25
Q

Name two characteristics of a suspension mixture.

A
  1. It is heterogeneous
  2. It can be easily filtered.
26
Q

Blood, fog and milk are all examples of what type of mixture?

A

These examples are classified as colloids because they scatter light and cannot separate very easy .

27
Q

Cloudy mixtures can be classified as suspensions or colloids. How can you tell the difference between each type of mixture based on appearance?

A
  • When mixed, the substances in a suspension will separate from one another. This is usually due to different densities. In addition, suspensions are easy to filter/separate since the particles are “suspended”.
  • Colloids are difficult to separate, and they are acloudy mixture that scatters light. This is due to the light being reflected diffusely, and refracted throughout the mixture.
28
Q

Why does a colloid scatter light?

A

Colloids “scatter” light because of something known as the Tyndall Effect. The light is scattering due to the refraction of light rays between closely spaced particles.

29
Q

Compounds and elements are what type of matter?

A

They are pure substances.

30
Q

What type of mixture would Italian salad dressing be?

A

Suspension because the particles separate after resting. It can also be easily filtered.

31
Q

Provide examples of solutions that involve multiple states of matter. For example, a gas dissolved in a liquid, etc.

A
32
Q
A
  1. Water=liquid
  2. Oxygen=gas
  3. Ammonium Nitrate=solid
  4. Ethanol=liquid
  5. Mercury=liquid
33
Q

What are some examples of evidence of a chemical change?

A
34
Q

What was John Dalton known for?

A

Dalton put forward the first modern theory of atomic structure. Each element is composed of a particle called an atom. All atoms in a particular element are identical in mass, and no two elements have atoms of the same mass. For instance, all oxygen atoms have the same mass, which is different from the mass of chlorine atoms. Dalton’s model is sometimes called the “billiard ball model” because he thought of the tiny atoms as solid spheres.

35
Q

Explain the difference between:

  • Electrons
  • Protons
  • Neutrons
A
  • Electrons: negatively charged particles orbiting the atom.
  • Protons: positively charged particles found in the nucleus.
  • Neutrons: neutral particles found in the nucleus of the atom.
36
Q

What are valence electrons?

A

Valence electrons are the number of electrons in the outer shell of an atom. (Bohr Diagram)

***As we move down a group, the number of valence electrons remains the same, even though the number of shells increases. While valence electrons across a period incrementally climb by one, the number of shells remaining the same. The period number (row number, to remind you) in which an element can be found indicates the number of shells encircling its nucleus.

37
Q

What is atomic mass?

How is it measured?

A
  • *Atomic mass** is the mass of one atom of an element. Scientists were able to determine the average mass of an atom of other elements by comparing it with the mass of a carbon atom (which is
    12. 0).

Atomic mass is measured by atomic mass unit (arnu). It is the total number of protons and neutrons in an atom.

38
Q

Each horizontal row is called a _______ (numbered from 1 to 7).

Each vertical column forms a _______, of elements (numbered from 1 to 18). These _______ have similar chemical properties.

A

Each horizontal row is called a period (numbered from 1 to 7).

Each vertical column forms a group/family, of elements (numbered from 1 to 18). These groups have similar chemical properties.

39
Q

Where can I find the atomic number, and what does it represent?

A

The number above the element’s symbol on the left is the atomic number. It shows how many protons are in the nucleus of one atom of the element.

An oxygen atom, for example, always has eight protons. Because atoms are neutral, the number of protons equals the number of electrons.

40
Q

Explain the chemical properties of Group 1, (alkali metals).

A

Group 1 elements, not including hydrogen, are called the alkali metals. These are the most reactive of the metals. They react when exposed to air or water. As you move down the group, the reactivity increases.

41
Q

Explain the chemical properties of Group 2, (alkaline earth metals).

A

Group 2 elements are called the alkaline-earth metals. They react when exposed to air and water as well, but their reactivity is not as strong as that of the alkali metals.

42
Q

Explain the chemical properties of Group 17 (Halogens).

A

Group 17 elements are called the halogens. They are the most reactive non-metals. For example, chlorine is commonly used to sterilize the water in swimming pools, and bromine gas is so corrosive it can burn skin. These elements are reactive and can combine with other elements to form new substances with useful properties.

43
Q

Explain the chemical properties of Group 18 (Noble Gases).

A

Group 18 elements are the noble gases, the most stable and unreactive elements. In fact, It was long believed that noble gases could never combine with other elements. It wasn’t until 1962 when that idea was proved incorrect. Canadian chemist Neil Bartlett and his colleagues at the University of British Columbia synthesized the first noble gas compound, combining xenon, platinum, and fluorine to create a new substance.

44
Q

What is the difference between metals, non-metals, and metalloids?

A

Metals are shiny, malleable, and ductile. They also conduct electricity. Most of the periodic table is full of metal elements.

Non-metals can be a solid or a gas. Solid non-metals are dull, brittle elements. Non-metals, except carbon, do not conduct electricity.

Metalloids have both metallic and non-metallic properties.

45
Q

What is an ionic compound? What are some properties of ionic compounds?

A

Ionic compounds are pure substances formed as a result of the attraction between particles of opposite charges, called ions.

ex) NaCl (table salt) is formed from positively charged
sodium ions and negatively charged chloride ions.

Properties of ionic compounds include their high melting point, good electrical conductivity, and distinct crystal shape.

All ionic compounds are solids at room temperature.

46
Q

What are polyatomic ions?

A

Polyatomic ions are group of atoms acting as one.

For example, 1 atom of carbon and 3 atoms of oxygen form the polyatomic ion called carbonate or CO32-. When carbonate reacts with calcium ions, the product is calcium carbonate, or limestone (CaCO3).

47
Q

What are 2 rules to use when naming ionic compounds?

A

First, the chemical name of the metal or positive ion goes first, followed by the name of the non-metal or negative ion.

Second, the name of the non-metal negative ion changes its ending to ‘‘ide’‘. This is the reason that the chemical name for NaCl is not sodium chlorine, but sodium chloride.

There is one exception to these naming rules. Where negative ions are polyatomic ions, the name remains unchanged. Limestone’s chemical name therefore remains calcium carbonate.

48
Q

What is a molecular compound and what are some properties associated with them?

A

When two or more non-metals combine, a pure substance called a molecular compound is formed.

Molecular compounds can be solids, liquids, or gases at room temperature. They tend to be insulators, or poor conductors of electricity. They also have relatively low melting and boiling points because the forces between the molecules are weak.

Examples of molecular compounds include sugar, acetylene, and water.

49
Q

What is a chemical change?

A

A chemical reaction occurs when two or more substances combine to form new substances.

50
Q

Define the terms reactant and product. Provide an exmaple of a chemical reaction that includes the reactants/products.

A
  • The materials at the start of reaction are called the reactants. (substances being combined)
  • The new materials produced by the reaction are called products.
    ex) In a campfire, the burning wood undergoes a combustion reaction. In this case, the reactants are wood and oxygen. In campfire, the products are carbon dioxide and water, formed while energy is released.
51
Q

What is the difference between exothermic and endothermic reactions?

Provide an example of each type of reaction.

A

Exothermic =releases heat

ex) When you burn an object in the presence of oxygen, energy in
the form of heat is given off. Heat is also emitted when your body
metabolizes food.

Endothermic=absorbs heat energy

ex) temperature in the baking soda and vinegar reaction
dropped during and just after the reaction.

ex) chemical cold-packs found in first aid kits are another example of where an endothermic reaction.

52
Q

What are 3 types of chemical reactions that occur involving oxygen as a reactant?

A

Three reactions in which oxygen reacts with other substances are combustion, corrosion, and cellular respiration.

53
Q

What is combustion?

A

Combustion is a chemical reaction that occurs when oxygen reacts with a substance to form a new substance and give off energy.

ex) Fire. In burning, wood reacts with oxygen to give off heat and light and produce carbon dioxide and water.

54
Q

What is corrosion?

A

Corrosion is the slow chemical change that occurs when oxygen in the air reacts with metal.

An example of corrosion is rusting. Rusting occurs when iron reacts with oxygen to form iron oxide.

55
Q

What is cellular respiration? Provide the chemical equation(reactants and products).

A

Cellular respiration is chemical reaction that takes place in the cells in your body. Food (glucose) reacts with oxygen to produce energy, water, and carbon dioxide.

56
Q

What is the law of conservation of mass?

A

It states that matter is not created or destroyed in chemical
reaction.

For example, combining 24.3 of magnesium and 32.1 of
sulfur creates new substance called magnesium sulfide.

The law of conservation of mass predicts that the mass of the product will be the sum of these two masses: 56.4 g.

57
Q

True or False?

The law of conservation has been proven by performing multiple experiments. These experiments have been done in closed
systems, where no additional material is allowed to enter or leave.

A

True.

58
Q

Provide an example of an open system.

A

Adding 10 of Alka-Seltzer to 100 of water in
beaker causes carbon dioxide gas to be given off. When the reaction is complete, the mass of the products left in the beaker is only 106 g, not 110 g.

The carbon dioxide gas was also one of the products of the reaction, but it escaped from the open beaker into the air.

59
Q

What are 4 factors that can affect the rate of a chemical reaction?

A
  • the presence of catalyst
  • the concentration of the reactants
  • the temperature of the reactants
  • the surface area of the reactants
60
Q

What is the difference between a catalyst and an enzyme?

A

Catalysts are substances that speed up a reaction. (Can be found in both living/non-living things)

An enzyme is a type of catalyst that can only be found in living organisms.

Science 9 GTHS (5 decks)

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