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Grade 9 Science - Unit 1 “Atoms, Elements, and Compounds” Guide

LAB SAFETY

1. Understand the importance of WHMIS and lab safety (refer to WHMIS worksheet)

2. Know and use proper techniques for handling and disposing of lab materials (MSDS sheets)

INVESTIGATING MATTER / PROPERTIES OF MATTER

3. Define matter

4. Define physical properties and chemical properties of matter

5. List examples of physical and chemical properties:

a. Physical properties: colour, malleability, electrical conductivity, magnetism, luster, density, melting/boiling points, texture

b. Chemical properties: combustibility, reactivity

ATOMIC THEORY

6. Explain the difference between a law and a theory

7. Identify major changes in atomic theory up to and including the Bohr model

8. Describe the contribution of various scientists to the development of current atomic theory:

a. Early Greeks (Empedocles, Democritus, Aristotle)

b. John Dalton

c. J.J. Thomson

d. Ernest Rutherford

e. Neils Bohr

9. Describe Rutherford's experiment to test Thomson's atomic model and discuss it as an example of how new technologies continue further development of atomic theory

10. Use models in describing the structure and components of atoms

a. Define atom

b. Distinguish between protons, neutrons and electrons in terms of charge, relative mass and location in the atom

ELEMENTS

11. Define element

12. Identify and write chemical symbols for common elements:

a. Hydrogen

b. Sodium

c. Potassium

d. Magnesium

e. Calcium

f. Iron

g. Nickel

h. Copper

i. Zinc

j. Carbon

k. Nitrogen

l. Oxygen

m. Neon

n. Helium

o. Chlorine

p. Silicon

q. Silver

r. Gold

s. Mercury

t. Lead

13. Recognize that elements are represented by an internationally agreed upon system of symbols

ELEMENTS AND THE PERIODIC TABLE

14. Describe and explain development of periodic table

a. Identify the Periodic Table as a listing of all known elements

b. Describe Mendeleev's contribution to modern table

c. Distinguish between atomic number and atomic mass

d. Using atomic mass and atomic number for an element, determine the number of protons, electrons and neutrons

ORGANIZATION OF THE PERIODIC TABLE

15. Use the periodic table to develop grouping of elements based on similar characteristics including:

a. Metals

b. Non-metals

c. Metalloids

d. Alkali metals

e. Alkaline earth metals

f. Halogens

g. Noble gases

h. Transition metals

16. List properties of metals and non-metals including:

a. luster

b. malleability

c. electrical conductivity

d. ability to conduct heat

17. Define period and family

18. Provide examples of common properties which a family of elements share including:

a. Noble gases

b. Alkali metals

c. Halogens

d. Alkaline earths

THE PERIODIC TABLE AND ATOMIC THEORY

19. Compare their characteristics and atomic structure of common elements:

a. Define energy level, valence energy level and valence electron

20. Draw Bohr-Rutherford diagrams for elements 1 to 18

21. Identify the maximum number of electrons which exist in the first three energy levels

22. Make comparisons of energy level diagrams for elements from the same family (group)

CHEMICAL COMPOUNDS / NAMING CHEMICAL COMPOUNDS

23. Identify and write chemical formula of common compounds:

a. Define compound and identify whether a simple compound is ionic or molecular

b. Identify that a compound is represented by a combination of element symbols known as a chemical formula which indicates the proportion in which the elements are present

c. List chemical formulas for some common chemical ionic compounds including

i. Table salt or sodium chloride (NaCl)

ii. Calcium carbonate (CaCO3)

iii. Sodium sulfite (Na2SO4)

iv. Sodium hydroxide (NaOH)

d. Name simple ionic compounds using IUPAC rules

e. List chemical formulas for some common chemical molecular compounds including:

i. Sucrose or table sugar (C12H22O11)

ii. Carbon dioxide (CO2)

iii. Methane (CH4)

iv. Water (H2O)

f. Name simple molecular compounds using IUPAC rules

CHANGES IN MATTER AND EVIDENCE OF CHANGES IN MATTER

24. Distinguish between physical and chemical changes (recognize that chemical changes produce new substances (elements and compounds), but physical changes do not)

25. List examples of physical and chemical changes including

a. Physical: change of state, cutting, dissolving

b. Chemical: corrosion, fruit ripening, combustion

26. List evidence that a chemical change may have occurred:

a. Heat is produced or absorbed

b. A new colour appears

c. A precipitate is formed

d. A gas is produced

e. Process is difficult to reverse

27. Recognize that during a chemical change, elements are conserved but compounds are not

CHEMISTRY IN EVERYDAY LIFE

28. Provide examples where knowledge of chemistry has resulted in the development of commercial materials

29. Explain how society's needs can lead to developments in chemistry

30. Analyze the design of a technology and the way it functions (based on its impact on your daily life)

31. Make informed decisions about applications of science and technology taking into account environmental and social advantages and disadvantages (CORE STSE – Plastics and Modern Life)

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