Atomic Structure & Periodic Table

Question 1

an electron can exist only in certain fixed energy states, so the energy of an electron is ________

Answer 1

quantized

Question 2

Absorption or emission occurs when an electron moves from _____________.

Answer 2

one energy level (one orbit) to another

Question 3

model of the atom that says that the position of an electron is described by the probablility of its being at different points in space;
an orbital is the function describing the probability of finding an eelctron at different points in space

Answer 3

quantum mechanical model

Question 4

states that it is impossible to determine both the position and the momentum of an electron with complete accuracy at the same time
the more preceisly we know the position, the larget the uncertainty in momentum and vice versa

Answer 4

Heisenberg Uncertainly Principle

Question 5

4 quantum numbers that describe electrons

determine properties of an electron: energy, angular momentum, orbital, etc.

Answer 5

n
l
m(l)
m(s)

Question 6

quantum number the describes the energy shell
can have integral value of 1,2,3, etc.
the larger the value, the higher the energy level and the farther away it is from the nucleus in general
corresponds to rows on the periodic table

Answer 6

principal quantum number (n)

Question 7

quantum number that describes the shape of the subshell (s, p, d, or f)
integral values from 0 —> n-1
n=1 shell has only one subshell, where this = 0

Answer 7

azimuthal (angular) quantum number (L)

Question 8

number of orbitals in a subshell

Answer 8

= 2 * L + 1
Ex: s subshell: one orbital (2*L + 1 = 1) b/c L=0
p subshell: 3 orbitals
d subshell: 5 orbital
f subshell: 7 orbitals

Question 9

quantum number that describes the spatial orientation of the orbital
integer values from -L to +L
specifies the particular orbital within a subshell occupied by an eelctron

Answer 9

magnetic quantum number: m(L)

Question 10

quantum number for any electron can have only one of 2 values: + 1/2 and -1/2
regardless of the shll, subshell, or orbital, any electron can have only one of two values for this

Answer 10

spin quantum number: m(s)

Question 11

states that no two electrons in an atom can have the same four quantum numbers
electrons in the same orbital have the same n, L, and m(l) quantum numbers. they must have different spin quantum numbers, so each orbital can holy only 2 electrons max

Answer 11

Pauli Exclusion Principle

Question 12

orbitals of the same energy level

Answer 12

degenerate orbitals

Question 13

indicates the size of the atom
increases w/ principle quantum number down a group
decreases as you move across a period to the right

Answer 13

atomic radius

Question 14

largest atoms are in the _________ of the periodic table

Answer 14

lower left hand corner (opposite electronegativity)

Question 15

measure of the attraction an atom has for electrons in a chemical bond
i.e. how storng an atom holds onto its electrons
increases from L to R on the PT
increases from bottom to top
highest = Fluorine
excludes noble gases

Answer 15

electronegativity

Question 16

energy required to completely remove an electron from a gaseous atom or ion
similar trend to electronegativity
low when the ionization process results in a noble gas configuration
Ex: this is low for alkali metals b/c removing an electron would bring them to a full octet, noble gas config
Ex: this is high for noble gases b/c they want to “hold onto” their full valence shell configs

Answer 16

ionization energy (energy of ionization)

Question 17

energy that is released when an electron is added to a gaseous atom or ion
represents the easy with which an atom can accept an electron
increases w/ stronger pull of nucleus for electrons
similar trend to electronegativity

Answer 17

electron affinity