Gr. 9 Chemistry Review!!! 1

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Matter is anything that has mass and takes up space. Chemistry is the study of matter and the changes it undergoes. 9

The Particle Theory of Matter 1. All matter is made up of tiny particles that have empty spaces between them. 2. Different substances are made up of different kinds of particles. 3. Particles are in constant random motion. 4. The particles of a substance move faster as its temperature increases. 5. Particles attract each other. 10

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Classification of Matter 13

Solution a uniform mixture of two or more substances Pure Substance: a substance that is made up of only one type of particle Mixture a substance that is made up of at least two different types of particles Mechanical Mixture a mixture in which you can distinguish between different types of matter Solution a uniform mixture of two or more substances Alloy a solid solution of two or more metals 14

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Homework Questions Pg. 178 #1-10 21

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How would you describe your luggage? Physical Property a characteristic of a substance that can be determined without changing the composition of that substance. How would you describe your luggage? Answer: You would describe physical properties! 25

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Qualitative Property a property of a substance that is not measured and does not have a numerical value, such as colour, odour, and texture 27

Quantitative Property a property of a substance that is measured and has a numerical value, such as temperature, height, and mass 28

Common qualitative physical properties include: colour, odour, taste, and texture. 29

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Physical Change: a change in which the composition of the substance remains unaltered and no new substances are Produced. 31

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Questions Pg. 182 34

Ch. 5.3 – Chemical Properties 35

chemical property a characteristic of a substance that is determined when the composition of the substance is changed and one or more new substances are produced 36

chemical change a change in the starting substance or substances and the production of one or more new substances 37

Evidence of Chemical Changes • a change of colour—a new substance has formed that has a different colour than the original substance • a change of odour—a new substance has formed that has a detectable odour • bubbles are visible that are not caused by heating—a new substance is produced in the form of a gas • a new solid is seen—a new substance that is produced does not dissolve in the mixture and shows up as a solid; • a change in temperature or light—energy is released or absorbed 38

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Pg. 186 41

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Pg. 198 #1-6 43

What is the difference between an element and a compound. Explain and provide examples. 44

Pure Substances 45

Metals are found on the left side of the Periodic Table Metal an element that is lustrous, malleable, ductile, and conducts heat and electricity. Metals are found on the left side of the Periodic Table 46

They are found on the upper right side of the periodic table, Non-Metal an element, usually a gas or a dull powdery solid, that does not conduct heat or electricity. They are found on the upper right side of the periodic table, 47

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Found on the staircase line of periodic table Metalloid an element that has properties of both metals and non-metals. Found on the staircase line of periodic table 49

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Pg. 215 53

Patterns in the Periodic Table 54

Chemical Family a column of elements with similar properties on the periodic table 55

Classifying the Elements The periodic table displays the symbols and names of the elements along with information about the structure of their atoms. 56

Groups Periods Each horizontal row of elements is called a period. Columns of elements are called groups or families. Elements in each group have similar but not identical properties. For example, lithium (Li), sodium (Na), potassium (K), and other members of group IA are all soft, white, shiny metals. All elements in a group have the same number of valence electrons. Each horizontal row of elements is called a period. The elements in a period are not alike in properties. In fact, the properties change greatly across even given row. The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas. 57

Alkali Metals They are the most reactive metals. They have one valence electron They react violently with water. Alkali metals are never found as free elements in nature. They are always bonded with another element. 58

Alkaline Earth Metals They are never found uncombined in nature. Like alkali metals, they are also very reactive. They have two valence electrons. Alkaline earth metals include magnesium and calcium, among others. 59

Halogen Gases Halogens are highly reactive, and can be harmful (Chlorine and Bromine are used as disinfectants) They are the most reactive non-metals They have 7 valence electrons They include Fluorine, Chlorine, Bromine, Iodine Fluorine is the most reactive. Once it does react with something, it bonds so strongly that the resulting molecule is very inert and non-reactive to anything else. Eg. Teflon is fluorine bonded with carbon. 60

Noble Gases The column on the far right of the periodic table (Group 18) These are very stable and unreactive elements They are all gases at room temperature 61

Hydrogen The hydrogen square sits atop group AI, but it is not a member of that group. Hydrogen is in a class of its own. It’s a gas at room temperature. Its nucleus contains only one proton (no neutrons!) and it has only one electron Hydrogen only needs 2 electrons to fill up its valence shell. 62

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Label and colour the groups on your handout!! 65

Pg. 225 #1-6 66

Review

Question #3,6,9 Pg. 240

Electronegativity: is a measure of the attraction an atom has for electrons when it is involved in a chemical bond.

Electronegativity: Noble gases have no electronegativity because they generally do not bond.

Chemical Bonding!!! How two more more atoms join together to form a compound!!

Ionic bond the result of the transfer of one or more electrons from a metal onto a non-metal.

Ionic bond the result of the transfer of one or more electrons from a metal onto a non-metal. Example: NaCl (Table Salt) Draw Lewis Dot Diagrams for this reaction.

Example: NaCl (Table Salt) Draw Lewis Dot Diagrams for this reaction. Ion: An atom with a different number of electrons than protons. Therefore it is charged!!! More electrons = Negative Less electrons = Positive

Covalent (Molecular) Bonding: Bonding between non-metals consisting of two electrons shared between two atoms. In covalent bonding, the two electrons shared by the atoms are attracted to the nucleus of both atoms. Neither atom completely loses or gains electrons as in ionic bonding.

Draw a Lewis Dot Diagram for Hydrogen + Oxygen Example Water!! Draw a Lewis Dot Diagram for Hydrogen + Oxygen

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