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62 Cards in this Set
- Front
- Back
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AX2 |
LINEAR 180 |
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AX3 |
TRIGONAL PLANAR 120 |
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AX2E |
BENT 120 |
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AX4 |
TETRAHEDRON 109.5 |
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AX3E |
TRIGONAL PYRAMID <109.5 (107) |
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AX2E2 |
BENT <109.5 (104)
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AX5 |
TRIGONAL BIPYRAMID 90,120,180 |
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AX4E1 |
SEE-SAW 90,120,180 |
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AX3E2 |
T-SHAPED 90,180 |
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AX2E3 |
LINEAR 180 |
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AX6 |
OCTAHEDRAL 90,180 |
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AX5E1 |
SQUARE PYRAMID 90,180 |
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AX4E2 |
SQUARE PLANAR 90,180 |
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what are the properties of elements ? |
atomic radius, metallic character, electron affinity, ionization energy |
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What is the ionization energy trend? |
increases across the period decreases down the group |
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what is the electron affinity trend? |
gaining of an electron increases across the period decreases down the group |
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metallic character trend? |
decreases across the period increases down the group |
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atomic radius trend ? |
distance from the center to the outermost electron. decreases across the period ' increases down the group |
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what is the electron configuration trend ? |
1s 2s 2p 3s 3p 4s 3d 4p 4d |
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s sublevel has ___ orbitals and can hold ____ p sublevel has ___ orbitals and can hold ____ d sublevel has ___ orbitals and can hold ____ f sublevel has ___ orbitals and can hold ____ |
1,2
3,6 5,10 7,14 |
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what are the metalloids ? |
B, Si Ge, As, Sb, Te, At Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Astatine |
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What if an electron has a charge ? |
you add or subtract it to the overall number of valence electrons |
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cations radius is ____ than neutral atoms anion radius is ____ |
smaller larger |
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cations in neutral form ____ electrons anions in neutral form ___electrons |
lose gain |
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paramagnetic
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attracted by magnets (unpaired electrons) |
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diamagnetic |
not attracted by magnets ( don't have unpaired electrons) |
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how do you determine of atoms are paramagnetic or diamagnetic ? |
draw the electron configuration and see of they're unpaired electrons or not. in the structure (box)` |
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how do you calculate formal charge ? |
# of valence electrons- #of lone electrons- 1/2( #bonded electrons) |
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how do you find the valence electrons? |
they are the same as the group number |
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When comparing species with the same amount of electrons the _____species is the one with the ___________ |
Smallest is the one with the greatest # of protons. ex: Ca 2+ and K+ Ca2+=18e K+=18e k has greater radius than Ca2+ b/c Ca2+ has more protons(20) than K+(19) |
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which group has the lowest ionization energy ? |
1A |
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What are the types of bonds |
ionic( NM-M)------electrons transferred covalent (NM-NM)----electrons shared metallic (M-M)------electrons pooled |
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whats the only exception to the types of bonds? |
NH4 ( ) with nonmetal or polyatomic ion |
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what is the lewis bonding theory ? |
atoms bond b/c it results in more stable configuration. more stable= less potential energy |
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What is octet rule and the exceptions ? |
Atoms bond to lose,gain, or share 8 electrons exceptions, Li,H,Be, B |
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Whats the Lewis theory prediction for ionic bonding ? |
# of electrons on METAL atoms should LOSE, or a NONMETAL should GAIN in order to attain stable configuration/electron arrangement. |
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Predict the formula for calcium and chlorine ? |
CaCl2 |
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what are some properties of ionic compounds |
solid at room temperature high melting point >300C soluble in water' melting in liquid state conducts electricity solid state don't conduct electricity |
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Whats the Lewis theory for covalent bonds? |
share valence electrons with other atoms in order to achieve octet |
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What is the trend in Bonding? |
single>double>triple |
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polar covalent bond |
covalent bonding unlike atoms results in unequal sharing of the electrons |
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whats the electronegativity trend |
increases across the period decreases down the group Fluorine has the highest electronegativity 1 |
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if the difference in EN is 0 then |
its purely covalent |
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if different in EN is b/t 0.1-0.4 |
its non polar covalent |
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if difference in EN is b/t 0/5-1.9 |
polar covalent |
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if difference in EN is greater than 2 it is |
100% ionic
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what is resonance |
2 or more structures that are correct |
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whats a hybrid ? |
is the actual structure b/t the 2 resonance . b/t double and single bond |
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Lewis theory exceptions |
1. odd # of electrons 2. electron deficient molecule-central atom with octet not satisfied. ex:BeF2 3. Expanded octets P S Cl As Se Br Kr Sb Te I Xe |
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For a molecule to be polar it must |
1. be polar 0.4-2.0 2. have unsymmetrical shape |
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what is dipole moment |
overal unequal distribution of electrons across the entire molecule. |
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Linear bonds are |
NONPOLAR |
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Bent bonds |
UNEQUAL DIPOLE MOMENT POLAR BOND |
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TRIGONAL PLANAR WITH EQUAL DIPOLE MOMENT |
EQUAL MOMENT NONPOLAR |
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TRIGONAL PLANAR WITH UNEQUAL MOMENT |
POLAR |
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TRIGONAL PYRAMID |
ALWAYS POLAR |
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TETRAHEDRAL IS POLARITIES ARE EQUAL unequal ? |
non polar unequal =polar |
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molecular orbitals ? |
2 atoms approached the half-filled valence atomic orbitals on each atom would interact. |
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what is the hybridization trend ? |
s p p p d d |
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atoms with 4 electron groups around (bond or lone pair) |
will form sp^3 hybrid with tetrahedral geometry 109.5 |
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atoms with 3 electron groups around it |
trigonal planar 120 forms an sp^2 |
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atoms with 1 group ex: c-c will form |
sp hybridizations |
