SLIDE 1 Slide 1 / 112
This material is made freely available at www.njctl.org and is intended for the non-commercial use of students and teachers. These materials may not be used for any commercial purpose without the written permission of the owners. NJCTL maintains its website for the convenience of teachers who wish to make their work available to other teachers, participate in a virtual professional learning community, and/or provide access to course materials to parents, students and others.
Click to go to website: www.njctl.org New Jersey Center for Teaching and Learning Progressive Science Initiative
Slide 2 / 112
www.njctl.org
Structure of Matter and Its Properties Classwork and Homework
Slide 3 / 112
Classwork #1: What is Matter?
Slide 4 / 112
1 If you have one atom of Oxygen and you break it in half, would you still have Oxygen? Explain.
Slide 5 / 112
2 Draw a model of an atom labeling all of its parts. On your model, identify which parts have a positive or negative charge or have no charge.
Slide 6 / 112
3 Explain what would happen if an electron and a proton were brought near each other and then
- released. Why would this happen?
SLIDE 2
Slide 7 / 112
Homework: What is Matter?
Slide 8 / 112
4 How do we define “matter?”
Slide 9 / 112
5 Can you think of anything that is not matter?
Slide 10 / 112
6 What does it mean for a substance to be a “pure substance?”
Slide 11 / 112
7 What subatomic particle has a neutral charge?
Slide 12 / 112
8 Where are electrons found in the atom?
SLIDE 3 Slide 13 / 112
Classwork #2: How Do We Measure Matter?
Slide 14 / 112
9 For each item below, identify the appropriate unit of
- measurement. The choices for the unit of
measurement are: volume (V), weight (W), mass (M) or both mass and weight (MW).
A Amount of water in a pool B Force of gravity on an apple C Kilograms D Amount of matter in a stone E Newton F Measured with a graduated cylinder G Cubic meters
Slide 15 / 112
H Length x Width x Height I Amount of juice in an orange J Pounds K Depends on location in a gravitational field L Grams M Measured with a Scale N Liters
9 (continued) For each item below, identify the appropriate unit of
- measurement. The choices for the unit of measurement
are: volume (V), weight (W), mass (M) or both mass and weight (MW).
Slide 16 / 112
10 Rank your weight on the surface of each of these locations from greatest to least. Justify your ranking to the right of the table.
Location Ranking Moon Jupiter Mercury Earth
Slide 17 / 112
11 Describe how you would find the volume of the empty vase below. Note that the vase is too large to fit in a standard graduated cylinder.
Slide 18 / 112
Homework: How Do We Measure Matter?
SLIDE 4
Slide 19 / 112
12 How many grams would be in 10 kilograms?
Slide 20 / 112
13 A block has a mass of 10 kg on Earth and a weight of 60 lbs. What would its mass and weight be on the moon?
Slide 21 / 112
14 A box has a length of 10 cm, a width of 8.5 cm and a height of 5.5 cm. What is its volume?
Slide 22 / 112
15 An irregular object is placed in 50 mL of water and the water level rises to 72 mL. What is the volume of the object?
Slide 23 / 112
16 Explain why the following statement is incorrect and then correct it: The apple weighs 1 kilogram.
Slide 24 / 112
Classwork #3: Elements of the Periodic Table
SLIDE 5
Slide 25 / 112
17 What did Mendeleev use to organize his first Periodic Table of Elements?
Slide 26 / 112
18 What is the symbol for Magnesium?
Slide 27 / 112
19 Which element is represented by the symbol C?
Slide 28 / 112
20 What period is Hydrogen (H) located in?
Slide 29 / 112
21 What group is Sulfur (S) located in?
Slide 30 / 112
22 Pick another atom with similar characteristics for each of these elements:
A Fluorine (F) B Oxygen (O)
SLIDE 6
Slide 31 / 112
Homework: Elements of the Periodic Table
Slide 32 / 112
23 How is the modern Periodic Table of Elements arranged?
Slide 33 / 112
24 Use your Periodic Table to answer the following questions about Helium (He):
A Atomic number? B Element Symbol? C Atomic Mass? D Number of protons? E Period? F Group? G Number of electrons in outer shell?
Slide 34 / 112
25 Suppose an element had an atomic number of 52. How many protons would that element have?
Slide 35 / 112
26 Using your Periodic Table, what element has an atomic number of 65?
Slide 36 / 112
27 Using your Periodic Table, which element has more protons: Nickel or Iodine? How do you know?
A Nickel B Iodine
SLIDE 7 Slide 37 / 112
28 Which element is represented by the symbol W?
Slide 38 / 112
29 What period is Silver (Ag) located in?
Slide 39 / 112
30 What group is Xenon (Xe) located in?
Slide 40 / 112
31 Pick another atom with similar characteristics for each of these elements:
A Potassium (K) B Krypton (Kr) C Strontium (Sr) D Gold (Au)
Slide 41 / 112
Classwork #4: Physical Properties
Slide 42 / 112
32 An unidentified clear liquid substance is found in the chemistry lab. One of your lab partners claims it is simply water while the other thinks it is isopropyl alcohol.
A What physical properties would NOT be helpful in identifying the substance and why? B Explain which physical properties could be used to identify the substance and how you and your lab partners would test these physical properties.
SLIDE 8 Slide 43 / 112
33 Describe the physical properties of a tent that are important if you are going camping for the
- weekend. For each physical property described,
explain why it is important.
Slide 44 / 112
34 You are given a mixture composed of finely ground salt and pepper and coarse sand. Explain how the physical properties of each item can help you separate them.
Slide 45 / 112
Homework: Physical Properties
Slide 46 / 112
35 Explain what physical properties of metal would be a good choice of material for each of these products and why:
A Cooking Pot B Power lines C Refrigerator door
Slide 47 / 112
36 Describe how the difference between metals and nonmetals can be detected.
Slide 48 / 112
37 For each item below, choose the most appropriate
- term. In some cases, you may have more than one
term listed: compound (C), molecule (M), element (E)
A _____ Basic unit of an element B _____ Water C _____ Pure substance D _____ Smallest part of a compound E _____ O3 F _____ salt
SLIDE 9 Slide 49 / 112
G _____ Carbon H _____ Two or more elements chemically bonded together I _____ The subscripts in H20 J _____ C6H1206 K _____ one or more atoms that are chemically bonded together
37 (continued) For each item below, choose the most appropriate
- term. In some cases, you may have more than one
term listed: compound (C), molecule (M), element (E)
Slide 50 / 112
38 Write the name of the family that is described in a-g:
A Does not react with other elements B End in -ine C React by losing 2 electrons D Poor conductor of electricity E 1 electron in the outer shell F Contains many unstable elements that do not occur naturally on earth G Can be mixed with other metals to make alloys
Slide 51 / 112
39 CaCO3, CO2, CuSO4, NaHCO3 Rank the compounds listed above from greatest to least based on:
A The number of different elements. B The total number of atoms.
Slide 52 / 112
40 What is the ratio of Sodium (Na) to Chlorine (Cl) atoms in the chemical formula NaCl?
Slide 53 / 112
41 The ratio of Carbon to Oxygen atoms in Carbon Dioxide is 1:2. How would you write its formula?
Slide 54 / 112
42 The molecule commonly known as Acetylene (C2H2) is made up of what types of atoms (and how many of each)?
SLIDE 10 Slide 55 / 112
43 The molecule commonly known as Nutrasweet (C14H18N2O5) is made up of what types of atoms (and how many of each)?
Slide 56 / 112
Classwork #5: Density
Slide 57 / 112
44 Complete the table below. Show your mathematical work on another sheet of paper. A periodic table displaying the density of elements is provided to help you.
Mass (g) Volume(cm
3)
Density (g/cm3) Element 345.5 356.1 155.3 57.5 94.2 4.54 10.13 2.7 59.6 7.13 4.88 3.14 53.6 23
Slide 58 / 112
45 Can a sample of an element be identified by its mass alone? Why or why not?
Slide 59 / 112
46 Suppose you had samples of equal mass for every element on the periodic table.
A Which elemental sample would contain atoms that are the most closely packed together? Justify your answer. B The least closely packed? Justify your answer.
Slide 60 / 112
47 You have one 3g sample of Nickel and one 3g sample of Manganese.
A Which sample takes up more physical space? Justify your answer. B Would either sample float in water? Why or why not?
SLIDE 11 Slide 61 / 112
48 A graduated cylinder is filled with 50mL of water. A sample of gold with a mass of 39.5 grams is dropped into the water. What will be the new water level on the graduated cylinder? Justify your answer.
Students type their answers here
Slide 62 / 112
Homework: Density
For each question below, show your work and/or justify your answer.
Slide 63 / 112
49 What is the density of a piece of wood that has a mass of 25.0 grams and a volume of 29.4 cm 3?
Slide 64 / 112
50 I threw a plastic ball in the pool for my dog to
- fetch. The mass of the ball was 125 grams. What
must the volume be to have a density of 0.500 g/mL? (I want it to float of course!)
Slide 65 / 112
51 What is the mass of a 12cm 3 sample of pure silicon with a density of 9 g/cm 3?
Slide 66 / 112
52 A piece of wood that measures 3.0 cm by 6.0 cm by 4.0 cm has a mass of 80.0 grams. What is the density of the wood? Would the piece of wood float in water? (Hint: recall how to determine the volume of a rectangular shaped object)
SLIDE 12 Slide 67 / 112
53 A strand of gold-colored metal beads was measured to have a mass of 425 grams. The beads are placed in a graduated cylinder where the original water level was 10mL. After the beads are placed in, the new water level in the graduated cylinder is 58mL. Given the following densities, identify the metal:
Gold 19.3 g/mL Copper 8.86 g/mL Bronze 9.87 g/mL
Slide 68 / 112
54 An ice cube measuring 5.80 cm by 5.80 cm by 5.80 cm has a density of 0.917 g/mL. What is the mass?
Slide 69 / 112
55 The density of aluminum is 2.70 g/mL. If the mass
- f a piece of aluminum is 244 grams, what is the
volume of the aluminum in cm 3?
Slide 70 / 112
Classwork #6: States of Matter
Slide 71 / 112
For each image below, identify an example of each common state of matter. Be sure to include scientific evidence that justifies your identified
- examples. Also determine whether the solid
identified is crystalline or amorphous and justify your answer.
Slide 72 / 112
56 Root Beer Float Solid: Liquid: Gas:
SLIDE 13 Slide 73 / 112
57 Hot Air Balloons over a lake Solid: Liquid: Gas:
Slide 74 / 112
58 Ice lake Solid: Liquid: Gas:
Slide 75 / 112
59 Geyser Solid: Liquid: Gas:
Slide 76 / 112
Homework: States of Matter
Slide 77 / 112
Use the word/phrase bank below to complete the Venn Diagram.
Definite volume Particles slide past each other Particles vibrate in place Definite shape Cannot be compressed Matter Atoms Molecules Has mass Particles have highest energy H2O at 27°C No definite volume Amorphous No fixed Shape Crystalline Particles are very close together Particles are not very attracted to each other Fluid
Then, come up with two examples of each state
- f matter and write them in the correct place on the
Venn Diagram.
Slide 78 / 112
Solid Gas Liquid
SLIDE 14 Slide 79 / 112
Classwork #7: Changes of State
Slide 80 / 112
The diagram below shows the water cycle- the movement of water throughout the Earth. Study the diagram and then use it to complete the following questions.
Slide 81 / 112
60 Label the arrows that represent evaporation with the letter ‘E’. Describe what is happening in these locations in terms of the thermal energy and temperature of the water.
Slide 82 / 112
61 Label the arrows that represent condensation with the letter ‘C’. Describe what is happening in these locations in terms of the thermal energy and temperature of the water.
Slide 83 / 112
62 Label any area on the figure where freezing might
- ccur with an ‘F’. Describe what is happening in
these locations in terms of the thermal energy and temperature of the water.
Slide 84 / 112
63 Are there any areas on the figure where boiling may occur? If so, label these areas with a ‘B’ and explain why you think it could occur there.
SLIDE 15 Slide 85 / 112
64 At what locations will H20 molecules
A have the highest energy? Explain. B have the lowest energy? Explain.
Slide 86 / 112
65 According to the diagram, water is never added or removed from Earth’s system. Explain how this is possible.
Slide 87 / 112
Homework: Changes of State
Slide 88 / 112
66 Why is a substance’s melting point and freezing point the same? Explain your answer in terms of thermal energy.
Slide 89 / 112
67 What differences are there between the two types
Slide 90 / 112
68 How can you tell that water is boiling? How can you tell that water is evaporating?
SLIDE 16 Slide 91 / 112
69 For a-d, write E if the sentence is referring to Evaporation and C if it is referring to Condensation:
A _____ A substance changes from a liquid to a gas. B _____ More molecules are breaking free from a liquid than joining it. C _____ More molecules are joining together with a liquid rather than leaving it. D _____ Molecules of water vapor are colliding and sticking together in the air.
Slide 92 / 112
For #70-75, identify the state of matter of the substances below at room temperature. Plot and label 0°C, the melting point (MP), the boiling point (BP), and room temperature (RT, 20°C) on a number line.
Slide 93 / 112
70 Mercury MP -39 °C BP 357 °C
Students type their answers here
Slide 94 / 112
71 Nickel MP 1455 °C BP 2913 °C
Students type their answers here
Slide 95 / 112
72 Silicon MP 1414 °C BP 3265 °C
Students type their answers here
Slide 96 / 112
73 Bromine MP -7 °C BP 59°C
Students type their answers here
SLIDE 17 Slide 97 / 112
74 Chlorine MP -102°C BP -34°C
Students type their answers here
Slide 98 / 112
75 Zinc MP 420°C BP 907°C
Students type their answers here
Slide 99 / 112
Classwork #8: Chemical Properties
Slide 100 / 112
76 How do physical properties differ from chemical properties?
Slide 101 / 112
77 Where can the most reactive elements be found in the Periodic Table? Where can the least reactive elements be found?
Slide 102 / 112
Homework: Chemical Properties
SLIDE 18
Slide 103 / 112
For #78-86, label each of these properties as chemical (C) or physical (P). Explain your choice.
Slide 104 / 112
78 Density
Slide 105 / 112
79 Tendency to corrode
Slide 106 / 112
80 Odor (scent)
Slide 107 / 112
81 Boiling/Melting Point
Slide 108 / 112
82 Reacts with acid
SLIDE 19
Slide 109 / 112
83 Solubility (dissolves)
Slide 110 / 112
84 Flammability
Slide 111 / 112
85 Reacts with Oxygen
Slide 112 / 112
86 Texture
