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56 Cards in this Set
- Front
- Back
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Cation
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Positively charged atom and has fewer electrons than its neutral form.
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anion
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Negatively charged atom and has more electrons than its neutral form
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Isotopes
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2 atoms of the same element having a different number of neutrons
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Mass Number
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The total number of protons and neutrons in the nucleus. Isotopes have different mass numbers.
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Elements in the same ROW
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...are similar in size.
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Elements in the same COLUMN
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....have similar electronic and chemical properties.
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Atomic Number
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Number of Protons
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Bonding
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The joining of two atoms in a stable arrangement. Always leads to lowered energy and increased stability.
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Rule that governs the bonding process:
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Through bonding, atoms attain a complete outer shell of valence e-
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Ionic Bonds
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Result from the transfer of electrons from one element to another. Generally occurs when elements on the far left side of the periodic table combine with elements on the far right side. The resulting ions are held together by extremely strong electrostatic interactions.
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Compound (bonds)
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Has ionic or covalent bonds
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Molecule (bonds)
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Has only covalent bonds
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Predicted # of Bonds = ___________
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8 - (# of valence electrons)
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Arrow direction drawn in ionic compound points _____
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from e- rich (negative sign) to electron poor (positive sign)
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Formal Charge
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The charge assigned to individual atoms in a Lewis structure.
(#Valence electrons) - (# electrons owned) |
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Number of Electrons Owned
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(# electrons unshared) + 1/2(# electrons shared)
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Resonance Structures
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Two Lewis structures having the same placement of atoms but a different arrangement of electrons.
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Methanol
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CH4O
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Ethylene
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C2H4
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Exceptions to octet rule (hypervalence)
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B, and any atom 3rd row and on.
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Acetylene
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C2H2
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Bonds where there will be resonance
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∏𝜎∏
∏𝜎V ∏𝜎N V𝜎N |
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No vacancy
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N = lone pair; negative charge
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Vacancy
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V = empty orbital; neutral or positive charge
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A better resonance structure has:
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more bonds and fewer charges
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Placement of charges in Resonance Structures
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- charges on more elctronegative atom [N,O]
+ charges on more electropositive atom [B,C] |
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Bond Lengths
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Decrease across a row as the size of the elements decrease, and increase down a group.
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What are "groups" in VESPR theory?
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an atom or a LONE PAIR
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2 Groups
[VESPR] |
LINEAR
180° bond angle EX: H-BE-H |
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3 Groups
[VESPR] |
Trigonal Planar
120º bond angle EX: H - B - H | H |
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4 Groups
[VESPR] |
Tetrahedral
109.5º bond angle EX: H | H - C - H | H |
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5 Groups
[VESPR] |
Trigonal Bipyramidal
120º, 90º bond angles EX: NH4 with a lone pair |
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6 GROUPS
[VESPR] |
Octagagonal/Octahedral
90º bond angles |
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Cis
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same side
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Trans
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opposite side
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In Skeletal Structures, charge:
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- takes the place of one hydrogen
-represents # of lone pairs |
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Ground State
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lowest level of energy
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The more S character in hybridization:
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The stronger the bond
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+ charge indicates
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no lone pairs
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- charge indicates
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one lone pair
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Hydrogen has what orbital?
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1s
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sp3
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one 2s orbital & three 2p orbitals [4 spy hybrid orbitals]
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sp2
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one 2s orbital & two 2p orbitals [3 spy hybrid orbitals]
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sp
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one 2s orbital & one 2p orbital [2 sp hybrid orbitals]
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What hybridization if 2 groups around atom?
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SP
2 orbitals used so TWO SP hybrid orbitals |
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What hybridization if 3 groups around atom?
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SP2
3 orbitals used so three sp2 hybrid orbitals |
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What hybridization if 4 groups around atom?
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SP3
4 orbitals used so four spy hybrid orbitals |
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All C-H bonds are formed from:
[hybridized] |
SP3 - 1S
C H |
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The O - H bond is formed from:
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SP3 - 1S
O H |
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What hybrid orbitals overlap in a 𝜎 bond?
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two sp2 hybrid orbitals
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What hybrid orbitals overlap in ∏ bond?
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side-by-side overlap of two 2p orbitals
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What hybrid orbitals overlap in a C - C double bond?
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a 𝜎 bond, formed by end-on overlap of two sp2 hybrid orbitals
a ∏ bond, formed by side-by-side overlap of two 2p orbitals |
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Ethane
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C2H6
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Acetone
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C3H6O
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A bond is polar if:
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Difference in electronegativity b/t two atoms is 0.5 or greater.
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hypervalence
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artificial d3 orbitals
- why B, P, S form 5 bonds |
