bonding basics
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Bonding Basics. Bell Work 11/15. 6CF₄ How many Carbon atoms are in the above molecule. How many Flourine atoms are in the above molecule? C₆H₁₂O₆ How many Carbon atoms are in the above molecule. How many Hydrogen atoms are in the above molecule?. - PowerPoint PPT PresentationTRANSCRIPT
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Bonding Basics
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Bell Work 11/15
6CF₄1. How many Carbon atoms are in the above
molecule.2. How many Flourine atoms are in the above
molecule?
C₆H₁₂O₆3. How many Carbon atoms are in the above
molecule.4. How many Hydrogen atoms are in the above
molecule?
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• An atom that gains one or more electrons will have a negative charge.
• An atom that loses one or more electrons will have a positive charge.
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Ions• An atom that gains or loses one or more
electrons is called an ion.
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2 Types of Bonds
• Ionic Bond• Covalent Bond
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Ionic Bond• A chemical bond in which one atom loses an
electron to form a positive ion and the other atom gains an electron to form a negative ion.
In this example, will sodium have a positive or negative charge?
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2 Types of Ions
• A positive ion is called a cation• A negative ion is called an anion
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Polyatomic Ions• Polyatomic ions: ions that are made of more
than one atom– Ex. An ammonium ion is made of nitrogen and
hydrogen atoms.
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Covalent Bond• Atoms share one or more electrons with each
other to form the bond.
– Each atom is left with a complete outer shell.
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Covalent Bond
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• Double bond: two atoms share two pairs of electrons
Covalent Bond
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• Triple bond: atoms share three pairs of electrons
Covalent Bond
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• Atoms of some elements pull more strongly on shared electrons than do atoms of other elements. As a result, the electrons are pulled more toward one atom, causing the bonded atoms to have slight electrical charges.
– Polar bond: a covalent bond in which electrons are shared unequally
– Nonpolar bond: a covalent bond in which electrons are shared equally
Covalent Bond
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• Covalent bonds usually form between atoms of nonmetals.
• In contrast, ionic bonds usually form when a metal combines with a nonmetal.
Covalent Bond
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Chemical Formulas• Subscript: tells you the ration of elements in
the compound.– Ex. MgCl₂
• This means that for every magnesium ion there are two chloride ions.
– Ex. CaCO₃• This means one calcium, one carbon, and three oxygen
ions.
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• If no subscript is written, the number 1 is understood.– Ex. NaCl
• This means there is one chloride ion for every sodium ion (1 to 1 ratio).
Chemical Formulas
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– Superscripts are the big number in front of an atom or molecule. They tell you how many atoms there are of that element.
• Ex. 4H– This means four atoms of hydrogen.
Chemical Formulas
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– When a superscript is in front of a molecule, it multiplies the whole molecule.
• 3H₂O– Here there are 6 hydrogens and 3 oxygens
– Basically like this: HHO HHO
HHO
Chemical Formulas
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Naming Covalent Bonds1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 heptaa
8 octa
9 nona
10 deca
* Second element in ‘ide’ from
* Drop –a & -o before ‘oxide’
N2S4 dinitrogen tetrasulfide
XeF6 xenon hexafluoride
P2O5 diphosphorus pentoxide
SO3 sulfur trioxide