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Transfer of 1 or more electrons between atoms (cations and anions)
Held together by electrostatic force (opposite charges)
Elements = metallic and nonmetallic
chrystalline
solids at room temperature
conducts an electric current in the molten state (or dissolved in water)
Brittle
STRONGEST BOND (ninja)
high melting points
formula units
high boiling points
ex: titanium dioxide, cesium chloride, sodium chloride, salt |
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A pair of electrons is shared between 2 atoms
Some are gases, some are liquids, some are solids (solids = malleable)
Molecule
elements = nonmetallic
low melting point and boiling point
poor conductors
ex: water, ammonia, diatomic elements (HONClBrIF), methane, carbon monoxide |
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Attraction of the free-floating valence electrons for the positive charged metal ions (forces that hold metals together) AKA: Overlapping of valence electrons
Malleable
Ductile
Shiny
Medium boiling & melting points
good conductors
all METALS
tend to be solid at room temp
ex: chromium, gold, zinc |
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Share bonding electrons
Exist as molecules
Follow the octet rule |
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brittle
involve the transfer of electrons
form crystal structures
held together by electrostatic force
follow the octet rule |
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Good conductors
malleable
held together by electrostatic force
electron sea (free moving electrons around nucleus) |
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| how many electrons are shared by 2 atoms in a double covalent bond? |
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| how many electrons are shared by 2 atoms in a triple covalent bond? |
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| involved in chemical bonding |
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| Electrons and bonds are indicated in Lewis dot structures with... |
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| a valence electron that doesn't bond |
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| The central atom in a Lewis Dot Structure can never be... |
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| Halogens will N-E-V-E-R... |
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| 2 electron pairs or 4 total electrons |
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| 3 electron pairs or 6 total electrons |
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| If the ion is POSITIVE []+ |
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| If the ion is NEGATIVE []- |
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| So who goes in the middle?? |
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| Put the hydrogens (etc.) on the element with fewer valence electrons |
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| How do 2 nonpolar molecules attract one another? |
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| they form temporary dipoles that stick ("induced dipoles") |
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| What is the name of the intermolecular force where 2 nonpolar molecules attract one another? |
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| 2 polar molecules that are attracted to each other |
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| how do dipole-dipole forces arise between molecules? |
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| the partial positive end is attracted to the partial negative end of the other |
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| an intermolecular force that occurs between H-O, H-N, and H-F |
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| LDF (London Dispersion Forces) |
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Rank the following from lowest to highest anticipated boiling point:
C2H4, FCN, NH3, H3COCH3 |
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| Hydrogen, Boron, and anything below the second period |
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bonds on central atom: 2
lone pairs on central atom: 0 |
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bonds on central atom: 2
lone pairs on central atom: 0 |
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bonds on central atom: 2
lone pairs on central atom: 1 |
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bonds on central atom: 2
lone pairs on central atom: 2 |
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bonds on central atom: 4
lone pairs on central atom: 0 |
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bonds on central atom: 3
lone pairs on central atom: 0 |
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| shape: trigonal pyramidal |
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bonds on central atom: 3
lone pairs on central atom: 1 |
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| REMEMBER: Bond polarity must read: |
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1. Non-polar COVALENT
2. Polar COVALENT
3. (or ionic) |
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| move a double/triple bond without changing the structure/molecule |
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| all elements must have 8 electrons in their outer most energy level to be considered stable |
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designed to show valence electrons in an atom
(also used to show bonding b/w multiple atoms) |
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| VSEPR: Valence Shell Electron Pair Repulsion Theory |
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| electron pairs repel to be as far apart from each other as possible |
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| Stronger intermolecular force... |
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| higher boiling point. why? harder to break the force |
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| IMF: (from weakest to strongest) |
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| London dispersion forces, dipole-dipole, hydrogen bonding, ion-ion |
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