covalent bonding
DESCRIPTION
Covalent Bonding. Sharing on an atomic level. Why do Atoms bond?. Gain Stability Ionic bonds gain stability by gaining or losing electrons. What happens if the pull isn’t strong enough to take or give up an electron?. Covalent bonding Results from sharing valence electrons. - PowerPoint PPT PresentationTRANSCRIPT
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Covalent BondingSharing on an atomic level
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Why do Atoms bond? Gain Stability
Ionic bonds gain stability by gaining or losing electrons.
What happens if the pull isn’t strong enough to take or give up an electron?
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Covalent bonding Results from
sharing valence electrons.
The pull isn’t enough to take the electron away.
Forms a Molecule Two or more
elements bonded together.
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How many bonds
Group 17 Single bond To another non-
metallic element Group 16
2 single bonds
Group 15 3 single bonds
Group 14 4 single bonds
A single bond is formed when one pair of electrons is shared betweenTwo elements.
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The sigma bond Single bonds are
called sigma bonds
σ bonds can be the overlap between two s orbitals or two p orbitals or and s and p.
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Homework• For Friday please practice
drawing covalent bonds for the following
• On page 244 1-5• PH3
• H2S• HCl• CCl4• SiH4
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Multiple bonds The double bond Have you ever thought about the
difference between the oxygen we breath and ozone?
They both are made of only oxygen atoms, but they are different.
It has to do with how they bond.
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The difference is the double bond
O2 O3
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Why? How does it happen? Take the next minute and a half and talk
to your table partner about it. Ideas?
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A second option In ionic bonds it was about equalizing
charges. In covalent bonds it is about making paired
electrons If an atom is able to make a single bond
and they both still have an unpaired electron. Which makes more sense to have both of them try to find another atom or for them to pair again with each other?
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Triple bonds A bond that is formed by sharing three
pairs of electrons. This can only happen if all three pairs
are on the atom. N and C families
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Pi bond A σ bond was for a single bond A π bond is formed for any double or
triple bond. They look different because they cannot
occupy the same space.
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Shapes What is happening in the process of
bonding? Electrons are coming together. They are
all – charged and so they repel each other.
So they are going to get as far away from each other as possible and still stay connected to the atoms.
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So lets visualize Ionic bonds- Girls are Cations and Boys
are Anions. Every one has a 1 charge. Covalent bonds Girls are carbons and
Boys are hydrogens. Pair up
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Molecular structure and naming
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Moving from Lewis dot to Structural formula You have been using Lewis dot
structures and molecular formulas Now we simplify it with structural
formulas Structural formulas use symbols and
bonds to show relative position of atoms.
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Figuring out number of bonds Atoms that make the most connections
go in the center Determine the number of electrons
available for bonding Divide that number in half to find the
number of bonding pairs Use as many of your bonding pairs for
single bonds Remaining bonding pairs will make
double or triple bonds
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PracticeMolecular Formula Lewis Structure Structural Formula
PH3
CH4
CCL4
O2
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PracticeMolecular Formula Lewis Structure Structural Formula
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Resonance Structures Resonance is when more than one
structure can be written for a molecule or ion.
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Exceptions to the Octet rule Odd numbers of valence electrons
N+O2= how many total electrons? 5+ 6+6= 17 They cannot be paired up.
Suboctets A lone pair of electrons can be shared by
a group that doesn’t have a spot BH3 + NH3
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Expanded Octets When the atom forms more bonds and
shares more than eight electrons. PCl5 SF6
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Naming Covalent bonds Naming Gases Very few things stay gas at room temperature. But for those that do we name them by ending
their name with gas It is important for knowing how many elements
you are talking about. Oxygen gas means you have 2 atoms of
oxygen. Chlorine gas? Helium gas?
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Naming Molecules Binary compounds1. The first element in the formula is always
named first, using the whole element name.2. The second element in the formula is
named using the root and changing the end to ide.
3. Prefixes are used to indicate the number of atoms of each element that are present. Ex. Monoxide, dioxide, tetrafloride.
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Number of Atoms Prefix1 Mono- (Used only for oxygen)2 Di-3 Tri-4 Tetra-5 Penta-6 Hexa-7 Hepta-8 Octa-
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Naming Acids binary The first word has the hydro to name
the hydrogen part of the compound The rest of the first word consists of a
form of the root of the second element plus the suffix –ic.
The second word is acid. Hydrochloric acid HCl
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Naming Acids oxyacids First identify the oxyanion present. The
first word of an oxyacid’s name consists of the root of the oxyanion and the prefix(if it exists) and the suffix. Suffix ate is released with ic ite is replaced with ous
The second word is always acid Sulfuric acid H2SO4