1. 1 Science 10 Chemistry Unit Review

2. 2 Chemistry is the study of matter, its properties, composition and behavior

3. 3 Matter is anything that has mass and occupies space. All matter has physical and chemical properties.

4. 4 Physical Properties are those properties that cause a physical change in a substance are those properties that cause a physical change in a substance example: boiling point, density, malleability (can be shaped without breaking), and ductility (can be drawn into a thin flexible wire)example: boiling point, density, malleability (can be shaped without breaking), and ductility (can be drawn into a thin flexible wire)

5. 5 Chemical Properties are those properties that describe how substances react with each other in a chemical reaction to form a new substance with different properties are those properties that describe how substances react with each other in a chemical reaction to form a new substance with different properties example: reactive and inert (unreactive)example: reactive and inert (unreactive) Note: proof of a chemical reaction could be a change in colour, energy, state or odour. Note: proof of a chemical reaction could be a change in colour, energy, state or odour.

6. 6 Matter Can Be Classified Matter Pure Substances Elements Compounds Metals Non-metals Ionic Molecular Mixtures Heterogeneous Homogeneous

7. 7 Definitions Pure Substances - have fixed properties that do not vary. Ex. elements and compounds Pure Substances - have fixed properties that do not vary. Ex. elements and compounds Elements - any substances that contain only one type of atom. Ex. C (carbon) and Al (aluminum) Elements - any substances that contain only one type of atom. Ex. C (carbon) and Al (aluminum) Molecular elements - whose molecules consist of more than one atom of the same element. Ex. H 2 (g), S 8 (s). Molecular elements - whose molecules consist of more than one atom of the same element. Ex. H 2 (g), S 8 (s).

8. 8 Definitions Compounds - any substance that contains two or more kinds of atoms in fixed proportions. Ex. H 2 O Compounds - any substance that contains two or more kinds of atoms in fixed proportions. Ex. H 2 O can be broken downcan be broken down can be either ionic (made up of a metal and a non- metal) or molecular (made up of two or more non- metals)can be either ionic (made up of a metal and a non- metal) or molecular (made up of two or more non- metals)

9. 9 Definitions Mixtures - are made up of two or more different compounds and or elements close together. They do not have a constant composition and proportions may vary. Ex. air, coffee, soft drinks. Mixtures - are made up of two or more different compounds and or elements close together. They do not have a constant composition and proportions may vary. Ex. air, coffee, soft drinks.

10. 10 Definitions Heterogeneous mixtures - are also referred to as mechanical mixtures because they contain different types of substances and states that do not appear uniform. Ex. concrete, this room.Heterogeneous mixtures - are also referred to as mechanical mixtures because they contain different types of substances and states that do not appear uniform. Ex. concrete, this room.

11. 11 Definitions Homogeneous mixtures - have the same properties throughout. They appear uniform in properties and can not be filtered. Ex. solutions and alloys.Homogeneous mixtures - have the same properties throughout. They appear uniform in properties and can not be filtered. Ex. solutions and alloys.

12. 12 Science 10 - Chemistry Unit The Periodic Table

13. 13 developed by Mendeleyev developed by Mendeleyev by arranging elements according to atomic mass, he discovered the Periodic Law which is the foundation of the Periodic Table.by arranging elements according to atomic mass, he discovered the Periodic Law which is the foundation of the Periodic Table. Periodic Law - patterns of reactivity, behavior, and properties occur in families or groups of elements. Periodic Law - patterns of reactivity, behavior, and properties occur in families or groups of elements.

14. 14 Patterns in the Periodic Table Elements are organized according to four basic patterns: Elements are organized according to four basic patterns: atomic numberatomic number metals & non-metalsmetals & non-metals periodperiod group/familygroup/family

15. 15 1. Atomic Number refers to the number of protons in an atom. Protons are positively charged subatomic particles in the atom’s nucleus. refers to the number of protons in an atom. Protons are positively charged subatomic particles in the atom’s nucleus.

16. 16 2. Metals & Non-metals Metals left of staircaseleft of staircase good conductors of heat and electricitygood conductors of heat and electricity shinyshiny malleable & ductilemalleable & ductile form positive ionsform positive ions all except mercury are solids at SATPall except mercury are solids at SATPNon-metals right of staircaseright of staircase poor conductorspoor conductors non shinynon shiny brittle (solids)brittle (solids) form negative ionsform negative ions either solids, liquids, or gas at SATPeither solids, liquids, or gas at SATP SATP = Standard Ambient Temperature & Pressure

17. 17 3. Periods are the horizontal rows of elements whose properties change from metallic to non-metallic from left to right along the row. are the horizontal rows of elements whose properties change from metallic to non-metallic from left to right along the row.

18. 18 4. Groups/Families are the vertical columns in the main part of the table whose elements have similar chemical properties. They are numbered left to right #1 - 18. are the vertical columns in the main part of the table whose elements have similar chemical properties. They are numbered left to right #1 - 18.

19. 19 4. Groups/Families a. alkali metals - (group 1) a. alkali metals - (group 1) – react violently with water and get more reactive as you move DOWN the group –hydrogen is not a member.

20. 20 4. Groups/Families b. alkaline earth metals (group2) –light, reactive metals c. halogens (group 17) –extremely reactive non- metals –F2(g) is most reactive

21. 21 4. Groups/Families d. noble gases (group 18) –extremely low chemical reactivity or inert (very stable) e. lanthinides (At. #57-71) and actinides (At. # 89-103)

22. 22 4. Groups/Families f. representative elements - in groups 1,2, and 13-18 g. transition elements in groups 3-12 - exhibit a wide range of properties

23. 23 Science 10 Chemistry Unit Atomic Theory

24. 24 Matter is made up of atoms. Over the past several hundred years, there have been many models of the atom. The model that we use today is the Bohr model, which is named after Niels Bohr. Matter is made up of atoms. Over the past several hundred years, there have been many models of the atom. The model that we use today is the Bohr model, which is named after Niels Bohr.

25. 25 Parts of the Atom atoms consist of three subatomic particles, protons, neutrons, and electrons. atoms consist of three subatomic particles, protons, neutrons, and electrons. protons (p+) and neutrons (nº) are located in the nucleusprotons (p+) and neutrons (nº) are located in the nucleus electrons (e-) are located around the nucleuselectrons (e-) are located around the nucleus

26. 26 Parts of the Atom ParticleSymbolChargeMass(amu) protonp+1+1 neutronnºno chg.1 electrone-1-negligible It would take 1830 electrons to equal the mass of 1 proton or neutron.

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28. 28 Protons the number of protons identifies the element. This is the element’s atomic number. If this number changes then the element becomes something else. the number of protons identifies the element. This is the element’s atomic number. If this number changes then the element becomes something else.

29. 29 Protons in an atom, the number of electrons always equals the number of protons. This makes the charge on an atom equal to zero. in an atom, the number of electrons always equals the number of protons. This makes the charge on an atom equal to zero. e.g.. carbon has 6 p+ and 6e- = no chargee.g.. carbon has 6 p+ and 6e- = no charge

30. 30 Neutrons the number of neutrons in an atom can be calculated by subtracting the number of protons from the atomic mass. the number of neutrons in an atom can be calculated by subtracting the number of protons from the atomic mass. #nº= atomic mass - atomic number

31. 31 Neutrons isotopes - are atoms of an element that have the same number of protons but the number of neutrons will vary from atom to atom. isotopes - are atoms of an element that have the same number of protons but the number of neutrons will vary from atom to atom. Compare carbon -12 & carbon-14 Compare carbon -12 & carbon-14

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33. 33 Practice Assignment At. Mass At#t.# # of protons # of electrons # of neutrons Name lithium aluminum sulfur chlorine carbon nitrogen magnesium calcium

34. 34 Practice Assignment