1. Chemistry
Semester 1 Review

2. Today:
Please put your phones in the basket and sit in your assigned seat.
We will be reviewing for the final today so have your final exam study guides and your notebook and something to write with ready when the bell rings.

3. Review: You will be working with partners – you will be A, B, C, or D.
I will tell you to discuss the questions with either A, B, C, or D partner and I will time you for each question.
You will be earning participation points for talking and answering questions.

4. Question #1 state the SI units for length, mass, temperature, and time
Meter, gram, Celsius, second.
A explain to partner B and C explain to partner D the “ladder method” and how it works.
After 30 seconds, switch.

5. Question #2 Rules: Express numbers in Scientific Notation:
1) If the number is positive, you add zeros AFTER the decimal point.
2) If the number is negative, you add zeros BEFORE the decimal point.

6. Question #3
A) be able to convert from meters (m) to km, cm, mm, µm, nm (p.74)
convert km to meters
0.044 to meters = 44 meters.

7. Question #3
B) be able to convert from liters (L) to ml, cm3, and µl (p.75)
convert 15 cm3 in liters
15 cm³ is .015 L – remember cm³ is the same as mL

8. Question #3
C) be able to convert from kilograms (kg) to g, mg, and µg (p.76)
convert 750 dg in grams
750 dg would be 75 grams.

9. Question #4
convert ratios of units (for example, convert 7.21 g/cm3 into kg/m3
Always remember: if it on the top AND the bottom they cross out.
Review dimensional analyses before the final.

10. Question #1 Chapter 4 Define atom
An atom is the smallest unit of matter.
Discuss with your partner what the 3 subatomic particles of an atom are.

11. Question 3: What is the electrical charge of each subatomic particle?
Discuss with your partner what happens when you gain or lose electrons.

12. Question #5:
Discuss the structure of an atom according to the Rutherford model.
Draw on your paper what this would look like.

13. Question #6
Discuss with your partner what distinguishes atoms of one element from atoms of a different element?
Write down on your paper what is the difference between an atom of oxygen and a molecule of oxygen.

14. Question #7
Write on your paper what is an atomic number and what is a mass number?
Discuss with your partner where each one is located on the periodic table and how you can tell the difference between them.

15. Question #8
Discuss with your partner – how do you calculate the number of neutrons in an atom?
If you know number of protons, how can you find number of neutrons?
If you know the mass number, and number of neutrons, how can you calculate the number of protons?

16. Question #9 80
Discuss with your parnterFor the element ₃₅BR, what is the atomic number, the mass number, and the number of neutrons?
Now switch partners.

17. Question #10 Discuss with your partner: what is an isotope.
Write down 4 examples of isotopes.

18. Question #11
Discuss with your partner, why do isotopes have different mass numbers?

19. Question #12
Write down what the correct name of a row across the periodic table is called?
Give me 3 examples.

20. Question #13
Write down what the correct name for a vertical row on the periodic table is.
Give me 3 examples.

21. Exit slip:
Answer the question on the exit slip for a chance to win participation points!

22. Today:
Please put your phones in the basket and get out a piece of notebook paper and a pencil.
We are going to be reviewing like we did yesterday, but you will be timed.
Anytime I tell you to write something down, you need to.
When I tell you to discuss something, you need to.
You will be graded on your participation in class and the paper you turn in today NOT your study guide.

23. Question:
Take 30 seconds and discuss with your shoulder partner the following question: According to the Bohr Model of the atom, how are electrons positioned around the atomic nucleus?
Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.

24. Question #2
Write down on your paper the answer to the following question:
What is an atomic orbital?
A region of space in which there is a high probability of finding an electron.
Draw what you think an atomic orbital would look like.

25. Question #3
Take 30 seconds and discuss the following question with your partner: Each principal energy level has a corresponding number of sublevels (Table 5.1, page 131).
Level 1 has a 1s orbital, thus holds _____ total electrons
Level 2 has a 2s orbital and three 2p orbitals, thus holds _____ total electrons
2, 8
What would Level 4 have?

26. Question #4 Take 30 seconds and explain the following to your partner:
Name and explain the three rules that determine the electron configurations of atoms.
1) Aufbau principle – electrons occupy orbitals of lowest energy first.
2) Pauli exclusion principle – an atomic orbital may describe at most two electrons. (1s can only hold 2 electrons)
3) Hund’s rule – electrons occupy orbitals of equal energy, one enters each orbital until all the orbitals contain one electron with the same spin direction. (1 up, and 1 down).

27. Question #5
Write on your paper the order in which electrons fill orbitals, from the 1s sublevel to the 4p sublevel (p.133)
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p

28. Extension:
Draw on your paper the pyramid for fill electron configuration orbitals.

29. Question #6
Write the electron configuration for the following elements on your paper: Ca C Se P

30. Question #1 Chapter 6
Discuss with your partner what are the three classes of elements in the periodic table? (p.158)
Metals, nonmetals, and metalloids.

31. Question #2
Discuss with your partner what are the key characteristics of each of the three classes of elements?
Metals – good conductors of heat and electrical current.
Nonmetals – poor conductors of heat and electrical current.
Metalloids – generally has properties that are similar to metals and nonmetals. It may behave like either a metal or a nonmetal.

32. Question #3
Discuss with your partner what is the group number for the noble gases? What is significant about the electron configurations of all noble gases? (p.164) 8, they have a full octet valence shell.

33. Question #4
Write on your paper what are the group numbers for the representative elements?
1A – 7A

34. Question #5
Discuss with your partner what do the electron configurations of all elements in the same group (or family) have in common?
They all represent the same number of electrons in the element’s highest occupied energy level.

35. Today:
Put your phones in the basket and we are going to have a new seating chart.

36. Today: We are going to review like we have been all week.
We will pick up where we left off yesterday.
If you get out a piece of paper and participate in class discussions, you will earn participation points.

37. Question #6
Discuss with your partner why elements containing d and f sublevels all belong to group B families?
They are all transition metals, meaning their charge changes depending on what they are reacting with.

38. Question #7
Discuss with your partner ionization energy and electronegativity. Describe the relationship between them.
It is the energy required to remove an electron from an atom.
It is the ability of an atom to attract electrons when the atom is in a compound.

39. Question #8
Look at Figure 6.22 on page 178. Discuss with your partner the periodic trends for each of the following properties:
atomic size
ionization energy
Electronegativity
Atomic size – increase down a group and decreases across a period.
Ionization energy - tends to decrease from top to bottom within a group and increase from left to right across a period
Electronegativity values - tend to decrease from top to bottom within a group. It tends to increase from left to right across a period

40. Question #1
What are valence electrons? Why are they important?

41. Question #2
How do you draw electron dot structures for representative elements?

42. Question #3
What is the octet rule? How do atoms of representative elements obey the octet rule?

43. Question #4
What is a cation? What groups of elements tend to form cations?

44. Question #5
Why do atoms of elements in the same group tend to form cations with the same charge?

45. Question #6
What is the charge of a cation from group 1A? group 2A? group 3A?

46. Question #7
What is an anion? What groups of elements tend to form anions?

47. Question #8
What is the charge of an anion from group 5A? group 6A? group 7A?

48. Question #9
Why do atoms of elements in the same group tend to form ions with the same charge?

49. Question #10
What is an ionic compound? What kind of bond holds atoms together in an ionic compound?

50. Question #11
How do you predict the chemical formulas of ionic compounds (p.196)?

51. Question #12 What are the properties of ionic compounds?
Extension: List three examples of ionic compounds.

52. Question #13
Given an ionic compound, be able to identify the cation and anion that formed the compound

53. Question #14
Given a cation and an anion, be able to state the formula of the ionic compound they will form

54. Exit Slip: Answer the following question on your paper and turn it in.
Define an ionic compound and give me three examples of ionic compounds.

55. Homework:
Finish chapter 8 section of study guide.

56. Question #1
What are two examples of diatomic molecules?

57. Question #2
What is an example of a covalent bond?

58. Question #3
What is an example of a diatomic molecule with a triple covalent bond?

59. Question #4
What is an example of a polar covalent bond?

60. Question #5
What is an example of a nonpolar covalent bond?

61. Question #6
What is the electron dot structure for water?

62. Question #7
What is an example of an ionic compound?

63. Question #8
When do covalent bonds form?

64. Question #9
What is the electron dot structure for OH⁻?

65. Question #10
What is an example of a molecule that would have a single covalent bond?

66. Question #11
What are intermolecular attractions?

67. Question #12
What are dipole interactions?

68. Question #13
What are hydrogen bonds? When do they form?

69. Question #14
Which bond is more weak; ionic or covalent?

70. Question #15
How can you tell what type of bond a molecule has?