1. Chapter 1: The Science of Chemistry

2. Changes of Matter SI Units & Measurement DensityProperties of Matter Classification of Matter 10 20 50 40 30 20 50 40 30 20 30 20 10 30 40 50 40 30 20 10

3. Boiling water is an example of what kind of change? Changes of Matter 10 Physical.

4. Changes of Matter 20 Identify the two states of matter shown in the physical change below: liquid gas

5. Give an example of a chemical change and explain why it is a chemical change. Changes of Matter 30

6. Liquid water is frozen into ice. Describe the motion of water molecules in each state. Changes of Matter 40 Liquid: molecules slide past one another. They move more freely than solids, but less so than gases. Solid: molecules are very close together and organized. Vibration is their only motion.

7. Name all four indicators that suggest a chemical change has occurred. Changes of Matter 50 Color change, formation of a gas, formation of a precipitate, change in energy.

8. The quantity mass is represented by what symbol? SI Units & Conversions 10 m

9. What unit is associated with the quantity n? mole SI Units & Conversions 20

10. Every measurement has two parts/components. What are they? Quantity and unit. SI Units & Conversions 30

11. What is a derived unit and why do we need them? A combination of 2 or more units. Some quantities cannot be represented with only one unit. SI Units & Conversions 40

12. Why was the SI system developed? SI Units & Conversions 50 To unify all measurements worldwide.

13. Density 10 What is the formula for density? D = m/V

14. Density 20 Density may be found by calculating the slope of a line on a graph. What should the x and y axis be on these graphs? x = volume y = mass

15. Name a frequently used derived unit for density. g/mL or g/cm 3 Density 30

16. In order to calculate density, you must know m and V. One way to find V for a solid is by using a ruler. What is the other method? water displacement Density 40

17. Calculate the volume given the following: D = 1.35g/mL and m = 16.8g. Must show all work! Round to one decimal place. V = 12.4mL Density 50

18. What kind of property is flammability? chemical Properties of Matter 10

19. What is a physical property? A property that can be observed without changing the identity of the substance. Properties of Matter 20

20. Which of the following properties are physical: density, reacts with water, chemical stability, taste, and smell. density, taste, and smell Properties of Matter 30

21. How do we determine chemical properties? By trying to cause a chemical change/actually performing a test. Properties of Matter 40

22. Nails rust easily. Explain WHY this is a chemical property. In testing its ability to rust, the chemical identity of the nail is changed (it chemically reacts with oxygen). Properties of Matter 50

23. Mixtures can be further classified into two types. What are they? homogeneous and heterogeneous Classification of Matter 10

24. In which category would you classify a sample of lead (Pb)? element Classification of Matter 20

25. A glass of water (H 2 O) and a piece of magnesium (Mg) are both considered what? pure substances Classification of Matter 30

26. Consider a glass of tea without ice cubes, and a glass of tea with ice cubes. How would you classify each? Why? Before: homogeneous; the tea is evenly mixed (appears to be all one substance). After: heterogeneous; you can visibly distinguish the ice from the tea- they’re not uniformly mixed. Classification of Matter 40

27. Name a difference between mixtures and compounds. 1. Mixtures- physically mixed, compounds- chemically mixed. 2. Mixtures- amounts can vary, compounds- definite composition. 3. Mixtures do reflect properties of components, compounds do not. Classification of Matter 50