1. 2 pt 3 pt 4 pt 5pt 1 pt 2 pt 3 pt 4 pt 5 pt 1 pt 2pt 3 pt 4pt 5 pt 1pt 2pt 3 pt 4 pt 5 pt 1 pt 2 pt 3 pt 4pt 5 pt 1pt Chapters1-3Chapters 7-8Chapter 9Chapter 10Chapters4-5

2. What did alchemists contribute to the development of chemistry?

3. What is alchemists developed the tools and techniques for working with chemicals.

4. Explain why collaboration and communication are important in science.

5. What is when scientists collaborate and communicate, they increase the likelihood of a successful outcome.

6. How does a chemical change affect the composition of matter?

7. What is during a chemical change, the composition of matter always changes.

8. In a chemical reaction, how does the mass of the reactants compare with the mass of the products?

9. What is during any chemical reaction, the mass of the products is always equal to the mass of the reactants.

10. What determines the density of an object?

11. Density is an intensive property that depends only on the composition of a substance, not on the size of the sample.

12. What are three types of subatomic particles?

13. What is three kinds of subatomic particles are electrons, protons, and neutrons.

14. How does the Rutherford model describe the structure of atoms?

15. What is in the nuclear atom, the protons and neutrons are located in the nucleus. The electrons are distributed around the nucleus and occupy almost all the volume of the atom.

16. What are the three rules for writing the electron configuration of elements?

17. What is three rules—the aufbau principle, the Pauli exclusion principle, and Hund’s rule—tell you how to find the electron configurations of atoms.

18. How are wavelength and frequency of light related?

19. What is the wavelength and frequency of light are inversely proportional to each other.

20. How does quantum mechanics differ from classical mechanics?

21. What is classical mechanics adequately describes the motions of bodies much larger than atoms, while quantum mechanics describes the motions of subatomic particles and atoms as waves.

22. How can you describe the electrical charge of an ionic compound?

23. What is they are composed of ions, ionic compounds are electrically neutral.

24. How do chemists model the valence electrons in metal atoms?

25. What is the valence electrons of metal atoms can be modeled as a sea of electrons.

26. How is an electron dot structure used to represent a covalent bond?

27. What is an electron dot structure such as H:H represents the shared pair of electrons of the covalent bond by two dots.

28. How is a coordinate covalent bond different from other covalent bonds?

29. What is a coordinate covalent bond, the shared electron pair comes from one of the bonding atoms.

30. Explain how the VSEPR theory can be used to predict the shapes of molecules.

31. What is VSEPR theory, the repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far apart as possible.

32. Describe how to determine the names of binary ionic compounds.

33. What is to name any binary ionic compound, place the cation name first, followed by the anion name.

34. How do you write the formulas and the names of compounds with polyatomic ions?

35. What is write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges.

36. How are the formulas for acids determined?

37. What is use the rules for writing the names of acids in reverse to write the formulas for acids.

38. How are bases named?

39. What is bases are named in the same way as other ionic compounds—the name of the cation is followed by the name of the anion.

40. What two laws describe how chemical compounds form?

41. What is the ways are summed up in two laws: the law of definite proportions and the law of multiple proportions.

42. Describe how to convert between the mass and the number of moles of a substance.

43. What is use the molar mass of an element or compound to convert between the mass of a substance and the moles of a substance.

44. How do you calculate the percent by mass of an element in a compound?

45. What is the percent by mass of an element in a compound is the number of grams of the element divided by the mass in grams of the compound, multiplied by 100%.

46. How is the molecular formula of a compound related to its empirical formula?

47. What is the molecular formula of a compound is either the same as its experimentally determined empirical formula, or it is a simple whole- number multiple of its empirical formula.

48. What are three ways to measure the amount of something?

49. What is measure the amount of something by one of three different methods—by count, by mass, and by volume.

50. How is the atomic mass of an element related to the molar mass of the element?

51. What is the atomic mass of an element expressed in grams is the mass of a mole of the element.