1. 10/19/ ll ork
Complete all Bell Work for the week on a sheet of paper. Turn it in by Friday!!
1: What does the atomic number tell us about the number of electrons? How do you know?
2: What does the group number (for group A elements) tell us about the number of valence electrons?

2. The handle of this titanium mug was joined to the body by welding
The handle of this titanium mug was joined to the body by welding. At the welding temperature, titanium reacts with oxygen in the air, forming an oxide. The oxide makes the weld more brittle. Chemical properties, such as reactivity, depend on an element’s electron configuration.

3. Stable Electron Configurations
When is an atom unlikely to react?
When the _________ occupied energy level of an atom is _________ with electrons, the atom is __________ and not likely to react.
highest
filled
stable

4. Stable Electron Configurations
The chemical properties of an element depend on the number of valence electrons. An _________________is a model of an atom in which each dot represents a valence electron. The symbol in the center represents the nucleus and all the other electrons in the atom.
electron dot diagram

5. Stable Electron Configurations

6. Stable Electron Configurations

7. 10/19/ ll ork
Complete all Bell Work for the week on a sheet of paper. Turn it in by Friday!!
1: What does the atomic number tell us about the number of electrons? How do you know?
2: What does the group number (for group A elements) tell us about the number of valence electrons?

8. Stable Electron Configurations

9. Stable Electron Configurations

10. Stable Electron Configurations

11. Stable Electron Configurations

12. Stable Electron Configurations

13. Stable Electron Configurations

14. Stable Electron Configurations

15. Stable Electron Configurations
Noble gases are the ___________elements.
The highest occupied energy level of a noble gas atom is completely filled.
The noble gases have stable electron configurations with eight valence electrons (two electrons in the case of helium).
Elements tend to react to achieve electron configurations similar to those of noble gases.
most stable

16. Ionic Bonds
What is one way in which elements can achieve stable electron configurations?
Some elements achieve stable electron configurations through the ________________between atoms.
transfer of electrons

17. Ionic Bonds Transfer of Electrons
A chlorine atom has one electron fewer than an argon atom. _________one electron would give chlorine a stable configuration.
A sodium atom has one more electron than a neon atom. _________one electron would give sodium a stable configuration.
Adding
Removing

18. Ionic Bonds
When sodium reacts with chlorine, an electron is transferred from each sodium atom to a chlorine atom. Each atom ends up with a more stable electron arrangement than it had before the transfer.

19. Ionic Bonds
When sodium reacts with chlorine, an electron is transferred from each sodium atom to a chlorine atom. Each atom ends up with a more stable electron arrangement than it had before the transfer.

20. Ionic Bonds
When sodium reacts with chlorine, an electron is transferred from each sodium atom to a chlorine atom. Each atom ends up with a more stable electron arrangement than it had before the transfer.

21. Ionic Bonds
When sodium reacts with chlorine, an electron is transferred from each sodium atom to a chlorine atom. Each atom ends up with a more stable electron arrangement than it had before the transfer.

22. Ionic Bonds Formation of Ions
When an atom gains or loses an electron, the number of protons is _____________to the number of electrons.
The charge on the atom is not balanced, and the atom is not neutral.
An atom that has a net positive or negative electric charge is called an_______.
The charge on an ion is represented by a plus or a minus sign.
no longer equal
ion

23. Ionic Bonds
The ion that forms when a chlorine atom gains an electron has 17 protons and 18 electrons.
This ion has a charge of 1–.
The symbol for the ion is written Cl1–, or Cl– for short.
An ion with a negative charge is an _________.
Anions like the Cl– ion are named by using part of the element name plus the suffix _______. Thus, Cl– is called a chloride ion.
anion
-ide
Start HERE!

24. A sodium ion has 11 protons and 10 electrons.
Ionic Bonds
A sodium ion has 11 protons and 10 electrons.
The sodium ion has a charge of 1+.
The symbol for the ion is written Na1+, or Na+ for short.
An ion with a positive charge is a __________.
A cation uses the element name, as in the sodium ion.
cation

25. Ionic Bonds Formation of Ions
Scientists use ___________to compare the sizes of atoms of different elements. The radius of a sphere is the distance from the center of the sphere to its outer edge–half the diameter of the sphere.
Atomic radii are extremely small. They are expressed in units of picometers (pm). There are one billion (109) picometers in a millimeter.
atomic radii
Stop here and do PhET simulation

26. Ionic Bonds
This table shows the atomic radius and ionic radius for six metals and six nonmetals. You will use the data to relate the size of an element’s atoms to the element’s location on the periodic table and to compare the sizes of atoms and their ions.

27. Ionic Bonds
Using Tables Within a period, what happens to the atomic radius as the atomic number of the elements increases?

28. Ionic Bonds
Using Tables Within a period, what happens to the atomic radius as the atomic number of the elements increases?
Answer: Within a period, the atomic radius decreases as the atomic number increases.

29. Ionic Bonds
Using Tables Within Groups 1A, 2A, 6A, and 7A, what happens to the atomic radius of elements as the atomic number increases?

30. Ionic Bonds
Using Tables Within Groups 1A, 2A, 6A, and 7A, what happens to the atomic radius of elements as the atomic number increases?
Answer: Within these groups, the atomic radius increases as the atomic number increases.

31. Ionic Bonds
Inferring How does adding an occupied energy level affect the atomic radius? (Hint: Lithium is a Period 2 element and sodium is a Period 3 element.)

32. Ionic Bonds
Inferring How does adding an occupied energy level affect the atomic radius? (Hint: Lithium is a Period 2 element and sodium is a Period 3 element.)
Answer: When the next higher energy level is occupied, there is a significant increase in atomic radius.

33. Ionic Bonds
Comparing and Contrasting Compare the atomic and ionic radii for potassium (K), and for bromine (Br).

34. Ionic Bonds
Comparing and Contrasting Compare the atomic and ionic radii for potassium (K), and for bromine (Br). Answer: The ionic radius for potassium is much smaller than its atomic radius. The ionic radius for bromine is much larger than its atomic radius.

35. Ionic Bonds
Making Generalizations What happens to the radius of an atom when the atom loses electrons? When the atom gains electrons?

36. Ionic Bonds
Making Generalizations What happens to the radius of an atom when the atom loses electrons? When the atom gains electrons? Answer: With the loss of valence electrons, the radius decreases. With the addition of valence electrons, the radius increases.

37. Ionic Bonds
Relating Cause and Effect Explain the difference in size between a metal atom and its cation.

38. Ionic Bonds
Relating Cause and Effect Explain the difference in size between a metal atom and its cation. Answer: An energy level that was occupied is no longer occupied, and the size decreases.

39. Formation of Ionic Bonds
A particle with a negative charge will attract a particle with a positive charge.
A __________ bond is the force that holds atoms or ions together as a unit.
An ________ bond is the force that holds cations and anions together. An ionic bond forms when electrons are transferred from one atom to another.
chemical
ionic

40. Ionic Bonds Ionization Energy
Cations form when electrons gain enough energy to escape from atoms. The energy allows electrons to overcome the attraction of the protons in the nucleus.
The amount of energy used to remove an electron is called ________ energy. The _______ the ionization energy, the easier it is to remove an electron from an atom.
ionization
lower

41. Ionic Bonds
This figure shows two trends for ionization energy.

42. 10/21/ ll ork
Complete all Bell Work for the week on a sheet of paper. Turn it in by Friday!!
1: What is the electron dot diagram for the following atoms (Mg, P, F)?
2: What is the electron dot diagram for the following ions (Mg2+, P3-, F1-)?
3:The atomic radius (increases/decreases) from left to right? From top to bottom?

43. How does the structure of an ionic compound affect its properties?
Ionic Compounds
How does the structure of an ionic compound affect its properties?
Solids whose particles are arranged in a lattice structure are called crystals.
The properties of an ionic compound can be explained by the _______ attractions among ions within a crystal lattice.
strong

44. Ionic Compounds
Compounds that contain ionic bonds are ionic compounds, which can be represented by chemical formulas.
A _________________is a notation that shows what elements a compound contains and the ratio of the atoms or ions of those elements in the compound.
The chemical formula for sodium chloride, NaCl, indicates one sodium ion for each chloride ion in sodium chloride.
Chemical formula

45. Ionic Compounds
What is the chemical formula for magnesium chloride?

46. Ionic Compounds
What is the chemical formula for magnesium chloride?

47. Ionic Compounds
What is the chemical formula for magnesium chloride?

48. Ionic Compounds
What is the chemical formula for magnesium chloride? A magnesium atom cannot reach a stable electron configuration by reacting with just one chlorine atom. It must transfer electrons to two chlorine atoms. After the transfer, the charge on the magnesium ion is 2+ and its symbol is Mg2+.

49. Ionic Compounds
The formula for magnesium chloride is MgCl2. The 2 written to the right and slightly below the symbol for chlorine is used to show the relative numbers of atoms of the elements present.
Magnesium chloride is used to control dust on unpaved roads.
Stop here and do PBS simulation

50. Ionic Compounds Crystal Lattices
A chemical formula for an ionic compound tells you the _______ of the ions in the compound, but not how the ions are arranged.
If you looked at a sample of sodium chloride with a hand lens or microscope, you would be able to see that the pieces of salt are shaped like cubes.
The crystal shape is a clue to how the sodium and chloride ions are arranged in the compound.
ratio
Stop here?

51. Ionic Compounds
Ions in sodium chloride are arranged in an ______, three-dimensional structure.
Each chloride ion is surrounded by six sodium ions, and each sodium ion is surrounded by six chloride ions.
Each ion is ________ to all the neighboring ions with an opposite charge.
This set of attractions keeps the ions in ______ positions in a rigid framework, or lattice.
orderly
attracted
fixed
Start here!

52. Ionic Compounds
The structure and shape of a crystal are related: A In a sodium chloride crystal, each ion is surrounded by six oppositely charged ions.
B Sodium chloride crystals are shaped like cubes

53. Ionic Compounds
The ____ of an ionic crystal, for example, the cubic shape of a sodium chloride crystal, depends on the arrangement of ____ in its lattice.
The arrangement of the ions depends on the ____ of ions and their relative ____. Crystals are classified into groups based on the shape of their crystals.
shape
ions
ratio
sizes
Start here!

54. Properties of Ionic Compounds
The properties of sodium chloride are typical of ionic compounds.
Sodium chloride has a high melting point (801°C).
Solid sodium chloride is a poor conductor of electric current. When melted, it is a good conductor of electric current.
Sodium chloride crystals shatter when struck with a hammer.

55. 10/22/ ll ork
Complete all Bell Work for the week on a sheet of paper. Turn it in by Friday!! 1:

56. Ionic Compounds
The arrangement of particles in a substance is the result of two opposing factors: the _________ among particles in the substance and the ___________ of the particles.
The stronger the attractions among the particles, the ______ kinetic energy the particles must have before they can separate.
Ionic compounds have strong attractions between particles and _____ melting points.
attractions
kinetic energy
more
high

57. Ionic Compounds
For an ____________ to flow, charged particles must be able to move from one location to another.
Ions in a solid crystal lattice have fixed positions. Solid sodium chloride is a ____ conductor of electric current.
When the solid melts, the lattice ___________, and the ions are free to flow. Molten sodium chloride is an ________ conductor of electric current.
electric current
poor
breaks apart
excellent

58. Ionic Compounds
Hammer strikes crystal
When an ionic crystal is struck, ions are moved from their fixed positions. Ions with the same charge ____ one another and the crystal shatters.
repel
Ionic crystal shatters when struck.

59. Assessment Questions When is an atom stable?
when its electrons are evenly distributed through its energy levels
when its lowest occupied energy level is filled with electrons
when its highest unoccupied energy level is filled with electrons
when its highest occupied energy level is filled with electrons

60. Assessment Questions When is an atom stable?
when its electrons are evenly distributed through its energy levels
when its lowest occupied energy level is filled with electrons
when its highest unoccupied energy level is filled with electrons
when its highest occupied energy level is filled with electrons ANS: D

61. Assessment Questions
Which description applies to an element that has two valence electrons?
reactive metal
nonreactive metal
reactive nonmetal
nonreactive nonmetal

62. Assessment Questions
Which description applies to an element that has two valence electrons?
reactive metal
nonreactive metal
reactive nonmetal
nonreactive nonmetal ANS: A

63. Assessment Questions
How do sodium and chlorine both achieve stable electron configurations when they react?
An electron is transferred from the sodium atom to the chlorine atom.
An electron is transferred from the chlorine atom to the sodium atom.
Both atoms gain one electron.
Both atoms lose one electron.

64. Assessment Questions
How do sodium and chlorine both achieve stable electron configurations when they react?
An electron is transferred from the sodium atom to the chlorine atom.
An electron is transferred from the chlorine atom to the sodium atom.
Both atoms gain one electron.
Both atoms lose one electron. ANS: A

65. Assessment Questions
Why do ionic compounds tend to have high melting points?
Ionic compounds contain more than one element, which causes a high melting point.
Ionic compounds cannot absorb energy efficiently because they contain ions.
An ionic compound contains metal atoms that raise its melting point.
A strong electrical attraction means ions require a lot of energy to move apart.

66. Assessment Questions
Why do ionic compounds tend to have high melting points?
Ionic compounds contain more than one element, which causes a high melting point.
Ionic compounds cannot absorb energy efficiently because they contain ions.
An ionic compound contains metal atoms that raise its melting point.
A strong electrical attraction means ions require a lot of energy to move apart. ANS: D

67. Assessment Questions
The ratio of aluminum ions to chloride ions in aluminum chloride (AlC13) is 3:1. True False

68. Assessment Questions
The ratio of aluminum ions to chloride ions in aluminum chloride (AlC13) is 3:1. True False
ANS: F, 1:3