why are electrons important? - warren township schools bonding... · why are electrons important?...
TRANSCRIPT
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Why are electrons
important?
• Chemical bonding involves electrons in the
outermost energy level (valence electrons) .
• When chemical bonds are formed, atoms
gain, lose or share electrons to have 8
electrons in their valence level.
• Exception: He (duet rule)
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C would like to
N would like to
O would like to
Gain 4 electrons
Gain 3 electrons Gain 2 electrons
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Chemical bonds
• Atoms attempt to fill electron shells.
• When electrons are gained, lost or shared, an
attractive force is formed
called a BOND, which holds elements
together.
-Ionic bonds (metal & non metal)
-Covalent bonds (2 non metals)
-Metallic bonds (2 metals)
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Ionic Bonding
• Occurs between a metal and a non-metal.
• Electrons are moved from one atom to another.
• The charged particle that results is called an
ION.
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IONS
• When an atom loses (or gives away) its
electrons, it becomes a positively charged.
• This is known as a CATION.
• Metals commonly
form positive ions.
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IONS
Continued..
• When an atom gains electrons, it becomes
negatively charged.
• This is known as an ANION.
• Non metals commonly form
negative ions.
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Formation of Ions
from Metals
Positive ions form when the number of electrons are
less than the number of protons
Group 1 metals ion 1+
Group 2 metals ion 2+
Group 13 metals ion 3+
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Formation of
Sodium Ion
Sodium atom Sodium ion
Na – e Na +
2-8-1 2-8 ( = Ne)
11 p+ 11 p+
11 e- 10 e-
0 1+
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Formation of
Magnesium Ion
Magnesium atom Magnesium ion
Mg – 2e Mg2+
2-8-2 2-8 (=Ne)
12 p+ 12 p+
12 e- 10 e-
0 2+
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Typical Ions with
Positive Charges
(Cations)
Group 1 Group 2 Group 13
H+ Mg2+ Al3+
Li+ Ca2+
Na+ Sr2+
K+ Ba2+
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Learning Check
A. Number of valence electrons in aluminum
1) 1 e- 2) 2 e- 3) 3 e-
B. Change in electrons for octet
1) lose 3e- 2) gain 3 e- 3) gain 5 e-
C. Ionic charge of aluminum
1) 3- 2) 5- 3) 3+
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Solution
A. Number of valence electrons in aluminum
3) 3 e-
B. Change in electrons for octet
1) lose 3e-
C. Ionic charge of aluminum
3) 3+
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Formation of Ions
from Nonmetals
• In ionic compounds, nonmetals in 15, 16, and 17
gain electrons from metals
• Nonmetals gain electrons to achieve a stable octet
• Nonmetal ionic charge: -3, -2, or -1
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Fluoride Ion
unpaired electron octet
1 -
: F + e : F :
2-7 2-8 (= Ne)
9 p+ 9 p+
9 e- 10 e-
0 -1
ionic charge
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Ionic Bond
Properties
• Crystal lattice: repeating 3D pattern
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Ionic Bond
Properties
• Strong attraction between ions result in
brittleness.
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Ionic Bond
Properties
• High melting points & usually solid at room
temperature.
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Ionic Bond
Properties
• Soluble
• Good Conductors
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Ionic Bonds:
One Big Greedy Thief Dog!
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http://web.jjay.cuny.edu/~acarpi/NSC/salt.htm
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1). Ionic bond – electron from Na is transferred to Cl,
this causes a charge imbalance in each atom. The Na
becomes (Na+) and the Cl becomes (Cl-), charged
particles or ions.
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Oxidation
Numbers
• The number of electrons that an element can
lose, gain or share is called the
OXIDATION NUMBER.
• Some elements have more than one
oxidation number, example Fe +2 or Fe+3
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Formula Weights
Or
Molecular mass
• Formula weight is the sum of the atomic
masses.
• Example- CO2
• Mass, C + O + O
12.011 + 15.994 + 15.994
43.999
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Covalent
Bond • Between 2 or more nonmetal elements.
• Formed by sharing electron pairs.
• Smallest unit of a covalently bonded
compound is called: molecule
• Examples; O2, CO2, C2H6, SiC
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Covalent Bond
Properties
• Low melting point & boiling point
• They are not conductors at any state. .
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Electrons are shared but shared unequally
POLAR COVALENT
BONDS
H2O
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Polar Covalent Bonds
Unevenly matched, but willing to share
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polyatomic
ions
A covalently bonded group of atoms acting as one that have a positive or negative charge.
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Diatomic
Molecules
• Some elements exist in nature as covalent
bonds.
• Composed of only 2 elements
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Diatomic
Molecules
• Nonmetals called the “Heavenly 7”
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Heavenly 7
Mnemonic
• HONClBrIF The Chemistry Goose
• Pronounced “Honk-Cool-Brief”
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Metallic
Bond
• Formed between atoms of metallic elements
• Metal atoms become cations surrounded by
a pool of electrons
• Good conductors at all states, lustrous, very
high melting points
• Examples; Na, Fe, Al, Au, Co
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Metallic Bonds:
Mellow dogs with plenty of bones to go around.
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Metallic Bond
Attraction between a metal cation and
shared electrons.
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Metals Form
Alloys
• Metals do not combine with metals.
• They form alloys which is a solution of a metal in a metal.
• Examples are steel, brass, bronze and pewter.
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Practice
• Compute the mass of the following compounds
round to nearest tenth & state type of bond:
• NaCl;
• 23 + 35 = 58; Ionic Bond
• C2H6;
• 24 + 6 = 30; Covalent Bond
• Na(CO3)2;
• 23 + 2(12 + 3x16) = 123; Ionic & Covalent
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The End