1. Define Physical Change

1. 1. Define Physical Change Physical changes occur when objects undergo a change that does not change their chemical nature.

2. 2. Define Chemical Change • A chemical change produces a new substance. Examples of chemical changes include combustion (burning), cooking an egg, rusting of an iron pan, and mixing hydrochloric acid and sodium hydroxide to make salt and water.

3. 3. Define Physical property • Physical properties can be observed without changing the type of matter. Examples of physical properties include: texture, shape, size, color, odor, volume, mass, weight, and density.

4. Hydrogen and oxygen react to make water A match burns A tree is cut down Sodium reacts with water to make sodium hydroxide Rusting of iron Boiling of water Digestion of food Boiling an egg. Melting of ice Circle the chemical changes

5. 5. Circle the statements which state a physical property. The boiling point of water is 1000 C The density of ice is lower than liquid water Water reacts violently with sodium Hydrogen burns with a popping sound. The color of Copper compounds is blue.

6. 1. The correct answer is D .The properties of shale do not change when it shatters.

7. 2. B. Separating the water into its elements –freezing water, calculating the density of water, or dissolving sugar in water do not change the properties of water.

8. 3. D. In rusting, the metal combines with other atoms.

9. Density                       Mass                                                  m             Density = --------------     or    D = -------                                                 Volume                         v Adjust the density formula and solve the problems below:    Mass=dxv                                                               

10. Viscosity Viscosity is the resistance of a fluid to flow. Honey is more viscous than water. www.oil-check.com

11. What happens to the viscosity of a liquid when it is heated? • Viscosity decreases when temperature is increased. Hot honey flows faster than cold honey.

12. Buoyancy is an upward force that keeps things afloat. www.fas.harvard.edu/.../CokeCanBuoyancy002.jpg

13. The density of water is 1.00g/ml. Water is more dense than oil so forms a layer below oil. http://www.csiro.au/files/images/paao.jpg www.dmturner.org

14. 1.  The density of silver is 10.49 g/cm3.  If a sample of pure silver has a volume of 12.993 cm3, what is the mass? Density = 10.49 g/cm3 Volume= 12.993 cm3, Mass= DXV 10.49g/cm3 x 12.993cm3 =136.3 g

15. A pipette is filled to 12 mL of sulfuric acid at 250 C and has a density of 1.83 g/mL. According to this information, what is the mass of this sulfuric acid solution? Sometimes a question will give you too much information. Focus on what you are looking for – Mass Mass = Density x volume =1.83g/ml x 12ml =21.96 g= 22.0g

16. Density of water is 1g/ml. If an object floats in water it’s density should be less than 1g/ml. The only object that has adensity less than 1 is D. D= M/V = 60g/65cm3 =.92g/cm3

17. If a graphic is given, look at it carefully. In order to calculate mass, you need density and volume. Mass = density x volume = 1.23g/ml x 19.4ml=23.9 g

18. 4. A block of gold has a volume of 800 cubic centimeters and a density of 19.3g/cm3 and the block is divided into two equal blocks. What is the density of the two smaller blocks? The density does not change when something is cut in half. The density of the two smaller blocks will also be 19.3 g/cm3

19. H -VISCOSITY

20. D. Decreases the viscosity

21. C. The density of liquid 3 is greater than density of liquid 2.

22. Elements Compound and Mixtures Circle the mixtures and underline the elements from the following list. Air Sodium Chloride Copper Water Bread CaCl2 Na

23. 2. What is the difference between an element and a compound? An element is made up of only one kind of atom. A compound is made of two or more elements combined together in a fixed ratio. http://www.physicalgeography.net/fundamentals/images/compounds_molecules.jpg

24. A. An element cannot be physically separated into other substances.

25. F- Compounds

26. Define atomic number: __Atomic number is the number of protons in the nucleus of an atom. Lead has 82 protons in it's nucleus and so the atomic number of lead is 82.

27. Which subatomic particles are present in the nucleus of an atom? Protons and neutrons are present in the nucleus of an atom.

28. Which of the sub atomic particles determines the identity of an element? Proton

29. What does an atom lose when a positive ion is formed? _____________ An atom loses an electron to form a positive ion.

30. Bohr models • Sodium Group : 1 Valence electrons : 1 Ion formed : +1 Atomic structure

31. Chlorine Group : 17 Valence electrons : 7 Ion formed : -1 Atomic structure

32. Neon Group : 18 Valence electrons : 8 Does not lose or gain electrons Atomic Structure

33. Sulfur Group : 16 Valence electrons : 6 Ion formed : -2 Atomic structure

34. Sodium will lose one electron to attain noble gas configuration.

35. Chapter 1 Metals, Nonmetals and Metalloids on the Periodic Table

36. Metals Located on the ______ side Form ________ Conduct heat and electricity Shiny appearance ________ ______ left cations Malleable Ductile

37. Non-metals • Located on the RIGHT side of the periodic table (except for ___________) • Form _______ • poor conductors of heat and electricity • Many are _____ at______________ HYDROGEN ANIONS GASES ROOM TEMPERATURE

38. Metalloids located __________ the metals and non-metals Have properties of both metals and non-metals ______ at room temperature IN BETWEEN SOLIDS SOLIDS

39. Metal/Nonmetal 1. Which of the following elements is a metal? • oxygen • calcium • Antimony • hydrogen

40. 2. Which of the following is not a metal? • Magnesium • Mercury • Silicon • Aluminum

41. Periodic Table and Trends 1. Which element has properties that are chemically most similar to the element Se? Cu Te Br Sc Te is in the same group as Se and so would be chemically similar to it.

42. 2. Define mass number- Mass number is the total number of protons and neutrons in the nucleus of an atom.

43. 3. Which groups of atoms are the most chemically similar? C, N, O C, N, P N, P, As Ge, As, S N, P and As belong to the same group and therefore are most chemically similar.

44. 4. The elements in the second vertical column of the periodic table are called? Alkaline earth metals

45. 5. Which of the following elements are in the same group as Boron? • Gallium • Nitrogen • Silicon • Aluminum

46. 6. Which of the following elements is most likely to donate an electron? Strontium Sodium Carbon Neon

47. 7. The elements of which group in the periodic table are most resistant to forming compounds ______________ Noble gases Noble gases have 8 valence electrons; their outer energy levels are complete and so they do not react with anything and are resistant to forming compounds.

48. 8. According to the periodic table what is the name of the group of elements that most readily accept electrons? Halogens – Group 17 have 7 valence electrons, they need only one more to complete their octet .This group therefore accepts electrons most readily

49. 9. Name four other elements that will have the same properties as Oxygen. • S, Se , Te , Po

50. 10. How many electrons should potassium gain or lose to attain a noble gas configuration? Potassium has 1 valence electron. When it loses the one valence electron, it now has 8 in its outer energy level.