chemistry chapter 6 - iss.k12.nc.us · pdf filegroup 1 = 1 electron ... •always lose...
TRANSCRIPT
![Page 1: Chemistry Chapter 6 - iss.k12.nc.us · PDF fileGroup 1 = 1 electron ... •ALWAYS LOSE ELECTRONS TO FORM CATIONS •Number of electrons lost can vary ... Chemistry Chapter 6 Author:](https://reader031.vdocuments.us/reader031/viewer/2022022422/5a9dba657f8b9a42488ca7a3/html5/thumbnails/1.jpg)
CHEMISTRYCHAPTER 6Ionic and Metallic Bonding
Covalent Bonding
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CHEMICAL BONDS
• A Chemical bond is a force that holds two or more atoms together.
• Chemical bonds involve (use) the valence electrons in the atoms.
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BONDS, CHEMICAL BONDS
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ELEMENTS IN A GROUP
•Behave similarly b/c they contain the same number of valence electrons
•Valence electrons are electrons in the highest occupied energy level
•Valence electrons determine an atom’s chemical properties
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VALENCE ELECTRONS
• Valence electrons of a representative element = group number
• Group 1A = 1 valence electron
• Group 4A (carbon) = 4 valence e- Group 5A (nitrogen) = 5 valence e-
• Group 6A (oxygen) = 6 valence e-
• Noble gases (group 8A) = 8 valence
• EXCEPT FOR HELIUM = 2 valence e-
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ELECTRONS IN CHEMICAL BONDS
•Are the valence electrons
•Electron dot structures are diagrams that show the valence electrons as dots around the symbol
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LEWIS STRUCTURES1) Find your element on the periodic table.
2) Determine the number of valence electrons.
3) This is how many electrons you will draw.
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LEWIS STRUCTURES
• Find out which group (column) your element is in.
• This will tell you the number of valence electrons your element has.
• You will only draw the valence electrons.
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GROUPS -REVIEW
•Each column is called a “group”
•Each element in a group has the same number of electrons in their outer orbital, also known as “shells”.
Group 1 = 1 electron
Group 2 = 2 electrons
Group 8 = 8 electrons
Except for He, it
has 2 electrons
•The electrons in
the outer shell are
called “valence
electrons”
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LEWIS STRUCTURES1) Write the element
symbol.
2) Carbon is in the 4th
group, so it has 4 valence electrons.
3) Starting at the right, draw 4 electrons, or dots, counter-clockwise around the element symbol.
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LEWIS STRUCTURES1) Check your work.
2) Using your periodic table, check that Carbon is in the 4th
group.
3) You should have 4 total electrons, or dots, drawn in for Carbon.
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LEWIS STRUCTURESOn your worksheet, try these elements on your own:
a) H
b) P
c) Ca
d) Ar
e) Cl
f) Al
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LEWIS STRUCTURESOn your worksheet, try these elements on your own:
a) H
b) P
c) Ca
d) Ar
e) Cl
f) Al
![Page 14: Chemistry Chapter 6 - iss.k12.nc.us · PDF fileGroup 1 = 1 electron ... •ALWAYS LOSE ELECTRONS TO FORM CATIONS •Number of electrons lost can vary ... Chemistry Chapter 6 Author:](https://reader031.vdocuments.us/reader031/viewer/2022022422/5a9dba657f8b9a42488ca7a3/html5/thumbnails/14.jpg)
LEWIS STRUCTURESOn your worksheet, try these elements on your own:
a) H
b) P
c) Ca
d) Ar
e) Cl
f) Al
![Page 15: Chemistry Chapter 6 - iss.k12.nc.us · PDF fileGroup 1 = 1 electron ... •ALWAYS LOSE ELECTRONS TO FORM CATIONS •Number of electrons lost can vary ... Chemistry Chapter 6 Author:](https://reader031.vdocuments.us/reader031/viewer/2022022422/5a9dba657f8b9a42488ca7a3/html5/thumbnails/15.jpg)
LEWIS STRUCTURESOn your worksheet, try these elements on your own:
a) H
b) P
c) Ca
d) Ar
e) Cl
f) Al
![Page 16: Chemistry Chapter 6 - iss.k12.nc.us · PDF fileGroup 1 = 1 electron ... •ALWAYS LOSE ELECTRONS TO FORM CATIONS •Number of electrons lost can vary ... Chemistry Chapter 6 Author:](https://reader031.vdocuments.us/reader031/viewer/2022022422/5a9dba657f8b9a42488ca7a3/html5/thumbnails/16.jpg)
LEWIS STRUCTURESOn your worksheet, try these elements on your own:
a) H
b) P
c) Ca
d) Ar
e) Cl
f) Al
![Page 17: Chemistry Chapter 6 - iss.k12.nc.us · PDF fileGroup 1 = 1 electron ... •ALWAYS LOSE ELECTRONS TO FORM CATIONS •Number of electrons lost can vary ... Chemistry Chapter 6 Author:](https://reader031.vdocuments.us/reader031/viewer/2022022422/5a9dba657f8b9a42488ca7a3/html5/thumbnails/17.jpg)
LEWIS STRUCTURESOn your worksheet, try these elements on your own:
a) H
b) P
c) Ca
d) Ar
e) Cl
f) Al
![Page 18: Chemistry Chapter 6 - iss.k12.nc.us · PDF fileGroup 1 = 1 electron ... •ALWAYS LOSE ELECTRONS TO FORM CATIONS •Number of electrons lost can vary ... Chemistry Chapter 6 Author:](https://reader031.vdocuments.us/reader031/viewer/2022022422/5a9dba657f8b9a42488ca7a3/html5/thumbnails/18.jpg)
LEWIS STRUCTURESOn your worksheet, try these elements on your own:
a) H
b) P
c) Ca
d) Ar
e) Cl
f) Al
![Page 19: Chemistry Chapter 6 - iss.k12.nc.us · PDF fileGroup 1 = 1 electron ... •ALWAYS LOSE ELECTRONS TO FORM CATIONS •Number of electrons lost can vary ... Chemistry Chapter 6 Author:](https://reader031.vdocuments.us/reader031/viewer/2022022422/5a9dba657f8b9a42488ca7a3/html5/thumbnails/19.jpg)
NOBLE GASES
•Unreactive in chemical reactions
•Octet rule: in forming compounds, atoms tend to achieve the electron configurations of a noble gas
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• Metallic elements tend to LOSE valence electrons
• Leave a complete octet in the next lowest energy level
• Nonmetallic elements tend to gain or SHARE electrons with another nonmetallic element to achieve a complete octet
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• Atoms are electrically neutral b/c the # of protons = # of electrons
• An ion forms as an atom or group of atoms loses or gains electrons
• A cation is a positive ion formed by the LOSS of valence electrons
• Name a cation the same as the atom (just add “ion”)
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CATIONS
• Differ chemically from their atoms
• Na atom explosive with water
• Na+ ion in NaClunreactive and harmless
• K atom explosive with water
• K+ ion in bananas harmless
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CATIONS
• Loses one valence electron to become a positively charged sodium ion (Na+ )
•Now, sodium has an electron configuration like neon
•Magnesium has 2 valence electrons
• LOSES 2 electrons to have a +2
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FORMATION OF POSITIVE IONS
• Lose one or more electrons
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TRANSITION METALS
• ALWAYS LOSE ELECTRONS TO FORM CATIONS
• Number of electrons lost can vary
• Ex: Iron (Fe) can lose 2 or 3 e-
• Fe+2 or Fe+3
• Transition metals can sometimes form pseudo-noble gas configurations• Silver (Ag) would have to lose 11 or gain 7 electrons. Instead, loses
it’s one 5s
• Then has 18e in outer most energy level
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ANIONS
•An atom or group of atoms with a negative charge. Atom must GAIN electrons to become negative.
• The name of the anion usually ends in “-ide”
•Chlorine (Cl) Chloride (Cl-)
•Oxygen (O) Oxide (O-2)
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ANIONS
• Easier for nonmetals to gain electrons vs. losing them b/c they have relatively full valence shells
• Halide ions: ions produced when halogens (like chlorine, fluorine) gain one electron
• All halide ions have a charge of -1
• Oxygen forms ions by gaining 2 electrons (O-2)
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FORMATION OF NEGATIVE IONS