exam 3

electron configuration

list of all electrons in an atom or ion going from low energy electrons to high energy electrons

orbitals

where do electrons reside?

s, p, d, f

4 types of orbitals

2

how many electrons can each orbital hold?

an electron in an atom

each box on the periodic table represents what?

energy level of electron

each row on the periodic table represents what?

type of orbital

each section of the periodic table represents what?

pauli exclusion principle

rule where an orbital can hold only 2 electrons, and they must have opposite spins

valid ground state electron configuration

where rules for filling orbitals are followed (the electrons are arranged in the lowest-energy orbitals possible)

hunds rule

rule where you must put 1 electron in each orbital before filling more

orbital configuration

shows how electrons are arranged within the individual orbitals of an atom

outermost shell

what shell has the highest energy level?

aufbau principle

rule where you start with the lowest energy level & go up (don’t move on from orbital until you fill that orbital)

half full or totally full

what is the most stable electron cloud?

anomalous electron configurations

electron clouds one way from being half full or totally full (configurations ending in d9, f6, f13, d4)

orbitals

electron probability maps, surfaces that contain 90% of the total electron probability

outermost shell

where do valence electrons live?

find outermost energy level, add up electrons with that number

how to find valence electrons from electron configuration?

group numbers (columns)

what on periodic table tells number of valence electrons?

1

how many orbitals in s in each energy level?

sphere

what shape is s orbital?

3

how many p orbitals at each energy level?

dumbell

what shape is p orbital?

nodal plane

what cuts through the orbital (electrons not found here, only found in the lobes)

2

nodal plan cuts p orbital into how many parts?

5

how many d orbitals in each energy level

clover

what shape is d orbital?

4

2 nodal planes cuts d orbital into how many parts? (the fifth orbital creates a cone shape)

7

how many f orbitals in each energy level?

complex, multilobed shape

what shape is f orbital?

8

3 nodal planes cuts d orbital into how many parts?

the number before orbital type

principal energy level in electron configuration is what?

right

atomic radius decreases as you go which direction on periodic table?

more protons are added, nucleus becomes positive, so it pulls the electrons more strongly

why does atomic radius decrease as you move to the right?

down

atomic radius increases as you go which direction on periodic table?

right

atoms get smaller going in which direction on periodic table?

effective nuclear charge increases (electrons want to move away, but protons pull them in, making the atom smaller but heavier)

why do atoms get smaller going right on periodic table?

down, left

atomic radii get larger going ____ and _____

ionization energy

the energy required to remove an electron from a neutral atom, forming a positively charged cation

high ionization energy

an electron is held tightly and its hard to remove

low ionization energy

an electron is held loosely and its easy to remove

increases going up and to the right

ionization periodic table trend

electron affinity energy

energy required to place an electron on a neutral atom (gain electron), forming an negatively charged anion

increases going up and to the right

electron affinity energy periodic table trend

energy is absorbed

positive electron affinity energy means what?

energy is released

negative electron affinity energy means what?

noble gases

what elements are the exception to electron affinity? (don’t need to gain anymore electrons?) (very low electron affinity)

electronegativity

the tendency for an atom to pull the electrons closer to it when it’s in a bond

increases going up and to the right

electronegativity periodic table trend

lewis dot structure

keeps track of how electrons are bonding or not bonding in molecules of polyatomic ions

visualizing 3d structure

what does drawing out lewis dot structure help with?

1. count up total valence electrons

-use group number for each element and add them

-if there’s a charge on the ion, add or subtract it (ex: 2- charge you would add 2, 2+ charge you would subract 2)

2. draw structure of molecule

-element written first goes in middle (hydrogen never in middle) (central atom is most electronegative)

3. add single bonds (single bond has 2 electrons)

4. place remaining valence electrons not accounted for in single bonds as lone pairs (go until octet rule is satisfied).

-place on outer atoms, then center atom

4b. if it’s a polyatomic ion, add square brackets and charge

5. if there are too few electrons to fill octet rule (usually on center atom), add double or single bonds

5b. if there are too many electrons, put extras on center atom as lone pairs (expanded octet)

lewis dot structure drawing instructions

resonance

more than one way to draw a lewis dot structure. double arrow indicates this (real 3d structure will be a hybrid of the two lewis dot structures)

ionic bonding

atoms are so different that one or more electrons are transfered to form oppositely charged ions (> 1.9 electronegativity) (ex: NaCl)

non polar covalent bonding

two identical atoms share electrons equally (<0.4 electronegativity) (ex: H - H)

polar covalent bonds

atoms are not so different that electrons are completely transferred, but enough that unequal sharing occurs

(0.4 < x < 1.9 electronegativity) (ex: H - F)

Valence Shell Electron Pair Repulsion theory (VSEPR)

Electron groups around a central atom repel each other, so they spread out as far apart as possible to minimize repulsions. The number of bonds and lone pairs around the central atom helps determine the 3D shape of the molecule.

linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral

types of electronic shapes (geometries) of molecules (depends on number of things attached to central atom - both bonds and lone pairs)

linear, 180

type of electronic shape with two things attached to central atom (bond or lone pair) and what is the degree angle between the two things?

trigonal planar, 120

type of electronic shape with three things attached to central atom (bond or lone pair) and what is the degree angle between the things?

tetrahedral, 109.5

type of electronic shape with four things attached to central atom (bond or lone pair) and what is the degree angle between the things?

trigonal bipyramidal, 90 & 120

type of electronic shape with five things attached to central atom (bond or lone pair) and what is the degree angle between the things?

octahedral, 90

type of electronic shape with six things attached to central atom (bond or lone pair) and what is the degree angle between the things?

number of bonds attached to central atom

types of shape of molecules just depend on what?

linear

molecule shape

trigonal planar

molecular shape

bent

molecular shape

tetrahedral

molecular shape

trigonal pyramidal

molecular shape

bent

molecular shape

trigonal bipyramidal

molecular shape

seesaw

molecular shape

t-shaped

molecular shape

linear

molecular shape

octahedral

molecular shape

square pyramidal

molecular shape

square planar

molecular shape

t-shaped

molecular shape

polarity

a lopsided distribution of electrons in a bond, molecule, or ion

bond polarity, molecule/ion polarity

two types of polarity

bond polarity

how unevenly the electrons are shared between two atoms in a chemical bond. It happens when the two atoms have different electronegativities (makes bonds asymmetrical which causes polarity)

dipole

what molecule has uneven distribution of electrical charge (has a slightly positive end and a slightly negative end)

polar

If molecular shape is asymmetrical, the molecule/ion is ____

nonpolar

If molecular shape is symmetrical, the molecule/ion is ____

less polar

similar electronegativities means what?

bonding continuum

a spectrum from equal sharing (non polar covalent) to unequal sharing (polar) to electron transfer (ionic)

covalent

what bond is usually nonmental + nonmetal

ionic

what bond is usually metal + nonmetal

nonpolar

any molecule shape that has the same atoms in all of the bonds and no lone pairs is ____ (symmetrical)

polar

all molecules with one lone pair are ____

individual shape

if molecule/ion has two lone pairs, look at ___________ to determine polar vs nonpolar

intermolecular forces

the attractive and repulsive forces between different molecules

intramolecular forces

the bonds inside a molecule or electrostatic attraction that forms the ionic compounds

dispersion force

when electrons get out of symmetry with the nucleus and forms a very short lived dipole (also called van der waals or london force) (everything has ______ force)

dispersion force

what is the weakest intermolecular force

increases

as molecular weight increases, dispersion forces _____

dipole dipole forces

what is the 2nd weakest/2nd strongest intermolecular force

dipole dipole forces

the attractive and repulsive forces for molecules with a permanent dipole (polar) (causes a more positive side and a more negative side, and those different sides repel/attract other molecules)

hydrogen bonding

what is the strongest intermolecular force

hydrogen bonding

special case & strongest case of dipole dipole forces. only occurs in compounds containing hydrogen bonded to highly electronegative elements N, O, F