1. Chapter 7 Ionic and Metallic Bonding 7.1 Ions 7.2 Ionic Bonds and
Ionic Compounds
7.3 Bonding in Metals
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2. Do Now: *THIS WILL BE COLLECTED* Name 2 alkali metals.
Valence Electrons
Do Now: *THIS WILL BE COLLECTED*
Name 2 alkali metals.
Name 2 alkaline earth metals.
Name 2 halogens.
Name 2 noble gases.
Write down 1 thing during your break that you can relate to Chemistry.
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3. Coming Up Today – Sec 7.1 Ions Tuesday – Sec 7.2 Ionic Bonding
Wednesday – Sec 7.3 Metals
Thursday – Review
Friday – Test on Chapters 6 & 7
Next Week – Presentations begin Tuesday /17
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4. Demonstrations Ions https://www.youtube.com/watch?v=xweiQukBM_k
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5. Ions An atom or group of atoms that has a positive or negative charge.
Atoms become ions when electrons are lost or gained.
Atoms can become cations or anions
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6. Cation – ion with a positive charge
Ions
Cation – ion with a positive charge
Metals tend to form cations.
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7. Anion – ion with a negative charge
Ions
Anion – ion with a negative charge
Nonmetals tend to form anions.
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8. Valence Electrons
Valence electrons - Electrons in the highest occupied energy level of an element’s atoms. These are the electrons involved in bonding.
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9. Electron Configurations in Groups
Determining Number of Valence Electrons
For representative elements, the group number tells you the number of valence electrons.
Group 1A elements have 1 valence electron
Group 4A elements have 4 valence electrons
Exception: Helium has only 2 valence electrons
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10. Determining the Number of Valence Electrons for the following atomsCs F O Xe He
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11. Determining the Number of Valence Electrons for the following atoms
Cs - 1
F - 7
O - 6
Xe – 8
He - 2
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12. Valence Electrons
Lewis Dot Structures
Diagrams that show valence electrons in the atoms of an element as dots.
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13. Interpret Data
Electron Dot Structures of Some Group A Elements
Period
Group 1A 2A 3A 4A 5A 6A 7A 8A 1 2 3 4
Notice that all the electrons within a given group (with the exception of helium) have the same number of electron dots in their structures.
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14. Draw electron dot structures for the following atoms
Valence Electrons
Draw electron dot structures for the following atoms Be Cs F O Xe He
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15. Valence Electrons
The Octet Rule
The octet rule states that in forming compounds, atoms tend to achieve the electron configuration of a noble gas.
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16. Valence Electrons
The Octet Rule
The octet rule states that in forming compounds, atoms tend to achieve the electron configuration of a noble gas.
An octet is a set of eight.
Atoms of noble gases (except helium) have 8 electrons in their highest occupied energy levels and an electron configuration of ns2np6.
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17. Valence Electrons
The Octet Rule
Atoms of metals tend to lose their valence electrons, leaving a complete octet in the next-lowest energy level.
Atoms of some nonmetals tend to gain electrons or share electrons with another nonmetal atom or atoms to achieve a complete octet.
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18. Atoms have 1 valence electron Lose 1 valence electron to form cation
Formation of Cations
Group 1A
Atoms have 1 valence electron
Lose 1 valence electron to form cation
Na Na+
–e–
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19. Formation of Cations
Group 1A Cations
Both the sodium ion and the neon atom have eight electrons in their valence shells (highest occupied energy levels).
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20. Group 2A Atoms have 2 valence electrons.
Formation of Cations
Group 2A
Atoms have 2 valence electrons.
Lose 2 valence electrons to form a cation
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21. Cations of Group 1A elements always have a charge of 1+.
Formation of Cations
Cations of Group 1A elements always have a charge of 1+.
Cations of Group 2A elements always have a charge of 2+.
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22. How does a cesium atom form a cation?
A. By losing 2 electrons
B. By gaining 1 electron
C. By losing 1 electron
D. By gaining 2 electrons
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23. How does a cesium atom form a cation?
A. By losing 2 electrons
B. By gaining 1 electron
C. By losing 1 electron
D. By gaining 2 electrons
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24. Formation of Anions
Atoms of nonmetals and metalloids form anions by gaining enough valence electrons to attain the electron configuration of the nearest noble gas.
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25. Formation of Anions
Chlorine atoms need one more valence electron to achieve the electron configuration of the nearest noble gas.
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26. Halide ions: ions produced when atoms of halogens gain electrons
Formation of Anions
Halide ions: ions produced when atoms of halogens gain electrons
All halogen atoms have 7 valence electrons and need to gain only 1 electron to achieve the electron configuration of a noble gas.
All halide ions (F–, Cl–, Br–, and I–) have a charge of 1–.
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27. Oxygen is in Group 6A, and an oxygen atom has 6 valence electrons.
Formation of Anions
Oxygen is in Group 6A, and an oxygen atom has 6 valence electrons.
An oxygen atom attains the electron configuration of neon by gaining two electrons.
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28. Formation of Anions
The name of an anion of a nonmetallic element is not the same as the element name.
The name of the anion typically ends in -ide.
Thus, a chlorine atom (Cl) forms a chloride anion (Cl–).
An oxygen atom (O) forms an oxide anion (O2–).
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29. Interpret Data Some Common Anions Name Symbol Charge Fluoride F– 1–
Chloride
Cl–
Bromide
Br–
Iodide I–
Oxide
O2– 2–
Sulfide
S2–
Nitride
N3– 3–
Phosphide
P3–
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30. Trends in Electronegativity
Electronegativity – ability of an atom of an element to attract electrons when the atom is in a compound.
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31. END OF 7.1
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