Matter has ____________ and ______________. 1. All ______________ is made of _____________.

1. mass volume Matter has ____________ and ______________. 1. All ______________ is made of _____________. 2. Mass is a _________________ of the amount of ____________. Mass- How to measure? Weight- How to measure? matter atoms measure matter triple-beam balance spring scale

2. States of Matter-Define and give molecular example of each.

3. Match the correct term to it’s picture. Find the picture and write it’s term near it. g/ml density Mass Triple-Beam Balance gram beaker Meter stick Graduated cylinder milliliter volume meter length

4. Matter is Made of Atoms-Write definitions for each. ATOMS CompoundS MIXTURES MOLECULES

5. MATTER yes no Can it be separated by physical means? MIXTURE PURE SUBSTANCE yes no yes no Is the composition uniform? Can it be decomposed by chemical means? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element

6. pr Protons, neutrons, electrons Are made of ATOMS Have a central nucleus Which contains Around which orbit Protons & neutrons electrons

7. Label each example of a heterogeneous and homogeneous mixture. Write a definition for each.

8. Name each element. H Si Al Li

9. 5. What period and family is the smiley face in? 6. What type of element is the sun shape? 7. What group/family is the heart in?

10. Complete these statements. Write the statements and fill in the blanks. 8. An atom that gains one or more electrons will have a ____________________ charge. 9. An atom that loses one or more electrons will have a ____________________ charge. 10. An atom that gains or loses one or more electrons is called an ____________.

11. Entry Task: What element is this? How many valence electrons does it have? What column would it be in? What is it’s atomic number? How many protons does it have?

12. Define density and list the tools used to measure it. The amount of mass in a given volume. Mass divided by volume Mass/volume = g/ml g/cm3 Triple beam balance Graduated cylinder ruler • Define the terms and give two examples of each: • Physical Property • Chemical Property Describes a substance Describes how a substance can change into another substance.

13. 2. Different compounds can be composed of… • The same elements in the same ratios • The same elements in different ratios • Only one element • No more than two elements Compounds have different properties from those of the .….

14. Look up Conservation of Mass or Law of Conservation of Mass in the textbook. • Write the definition. DEMO NaHCO3 + CH3COOH = H2O + CO2 + CH3COONa

15. An isotope is a form of an element with more or less than the common number of neutrons. Which of the following is an isotope for Uranium 92 with a mass of 238 .029? An element with a. 92 protons and 146 neutrons b. 93 protons and 146 neutrons c. 92 protons and 135 neutrons d. 146 protons and 92 neutrons What is an isotope? Answer in complete sentences.

16. Copy the chart into your lab book Homogeneous Heterogeneous Cannot be easily separated Both Come from atoms Elements or compounds Can be physically separated

18. A chemical bond formed when two atoms share electrons is called a(n) a. ionic bond. b. covalent bond. c. polyatomic bond. crystal bond. What is the greatest number of valence electrons an atom can have? a. 2 b. 3 c. 8 d. 12 A row across the periodic table is called a a. group. b. family. c. section. d. period. Which parts of the atom move around the nucleus? a. atomic mass units b. electrons c. protons d. neutrons

19. A solid is a state of matter that has a(n) a. indefinite volume and an indefinite shape. b. definite volume and a definite shape. c. definite volume and an indefinite shape. indefinite volume and a definite shape. An uncovered pot of soup is simmering on a stove, and there are water droplets on the wall above the back of the stove. What sequence can you infer has occurred? a. melting, then boiling b. freezing, then thawing c. evaporation, then condensation d. condensation, then vaporization Data plotted on a graph results in a line that slopes upward from left to right. This graph tells you that a. when one variable increases, the other variable increases. b. when one variable increases, the other variable decreases. c. when one variable increases, the other variable remains the same. d. both variables are decreasing. Copper, oxygen, and helium are examples of ____________________. elements

20. plasma In stars, matter exists in the ____________________ state, which is a gas-like mixture of free electrons and atoms stripped of their electrons. This type of bond is formed when a negative ion is attracted to a positive ion. Bond formed when electrons are transferred. Ionic Bond 17 2 How many atoms of a Group 17 element would be needed to react with one atom of a Group 2 element? Explain. 2

21. Atoms of Some Common Elements Element Atomic Number Mass Number Protons Neutrons Electrons Sodium 11 ? 11 12 ? Magnesium 12 24 12 ? 12 Aluminum ? 27 13 14 13 Phosphorus 15 31 ? 16 15 How many protons are in an atom of phosphorus? 15 Explain the difference between an ionic and a covalent bond. Use the terms: electrons transferred shared bond molecule crystal structure • Ionic bonds transfer electrons and make crystal structures. • Covalent bondsshare their electrons and tend to make molecules.

22. Explain the difference between an ionic and a covalent bond. Use the terms: • Ionic • covalent • electrons • Transferred • Compound • Metal • Non-metal • shared • bond • molecule • crystal structure • Ionic bonds transfer electrons and make crystal structures. These are compounds made between metals and non-metals. • Covalent bondsshare their electrons and tend to make molecules. These are made between non-metals.

23. Name the following substances as either pure, homogeneous or heterogeneous. heterogeneous pure heterogeneous homogeneous homogeneous pure

24. Changing An Atom Changing An Atom Changing An Atom Changing An Atom New element molecule ion isotope

25. Copy the charts and fill in the missing information. YOU CANNOT USE THE TEXTBOOK

26. Match the term to it’s definition. Freezing process of a liquid changing into a gas Melting process of a solid changing into a gas without going through the liquid phase Evaporation process of a liquid changing into a solid Condensation process of a solid changing into a liquid Sublimation process of a gas changing into a liquid

27. IONS GAIN-NEGATIVE LOSE+POSITIVE If the atom gains electrons it will have more electrons than protons. It will have a negative charge. If the atom loses electrons it will have more protons than electrons. It will have a positive charge.

28. Ionic Bonds-Transfer • Ionic bonds transfer electrons. • The metal element becomes a positive ion. • The non-metal element becomes a negative ion. I T

29. Covalent Bonds-Share • Covalent bonds share electrons. C S

30. Energy Endothermic • Energy in • Reactants  Photosynthesis 6CO2 + 6H2O + energy C6H12O6 + 6O2 • Drop in temperature Exothermic • Energy exits • Products C6H12O6 + 6O2  6CO2 + 6H2O + energy • Rise in temperature

31. Chemical Reactions

32. pH 7= Neutral Acids • Turn litmus red • Taste sour • Burning sensation • 0-6 Bases • Turn litmus blue • Taste bitter • Soapy/slippery • 8-14