unit one study guide key words and terms

Question 1

paired electron

Answer 1

means all two spin states of the orbital specified by three quantum numbers n, l and m are fully occupied by two electrons

Question 2

alkaline earth metals

Answer 2

group 2a metals, fairly reactive metals

Question 3

electron affinity

Answer 3

energy released when adding an electron

Question 4

Dalton

Answer 4

created Dalton’s law of partial pressure. A law stating that the sum of the partial pressures of each component in gas mixture equals the total pressure

Question 5

unpaired electron

Answer 5

electron that occupies an orbital of an atom singly, rather than as part of an electron pair

Question 6

J.J. Thomson

Answer 6

J.J. Thomson was born on December 18, 1856, in Cheetham Hill, England, and went on to attend Trinity College at Cambridge, where he would come to head the Cavendish Laboratory. His research in cathode rays led to the discovery of the electron, and he pursued further innovations in atomic structure exploration.

Question 7

electron density

Answer 7

measure of the probability of an electron being present at a specific location.

Question 8

what family of elements is mostly unreactive

Answer 8

nobel gases, all their valence electrons are full

Question 9

metalloids

Answer 9

aka semiconductors zig zag line intermediate electrical conductivity which can be changed and controlled usefull for manufacturing

Question 10

effective nuclear charge equation

Answer 10

Zeff= Z - S

Question 11

excited state

Answer 11

unstable state for an atom/molecule in which energy has been absorbed but not re-emitted, raising an electron from ground state into a higher energy orbital

Question 12

what is angular momentum QN aka, and what does it affect, what are the possible values

Answer 12

aka: subshell
affects: orbital shape

possible values: 0,1,2,3 or n-1

Question 13

what does m_l stand for, and what does it affect, possible values

Answer 13

magnetic quantum number, affects spatial orientation

possible values: -L,…-1,0,1,…L

Question 14

metals

Answer 14

left side/periodic table. good conductors/heat and electricity. malleable, can be drawn to wires (ductility) often shiny

Question 15

alkali metals

Answer 15

grop 1a elemetnys, highly reactive metals

Question 16

angular momentum quantum #

Answer 16

The angular momentum quantum number, l, (subshell) describes the shape of the orbital. l = 0, 1, 2, … , n – 1 The higher the value of l the higher the energy.

Question 17

energy level

Answer 17

light is a particle that moves like a wave. (everything moves like a wave) Only certain energy levels can exist. energy is quantized.

Question 18

transition metals

Answer 18

less easily predictable properties based on their position in the periodic table

Question 19

what does Zeff mean

Answer 19

charge “felt” by a valence electron

Question 20

order of electromagnetic spectrum

Answer 20

radio waves, microwaves, infrared waves, visible light, ultraviolet radiation, X-rays, and gamma rays

Question 21

principal quantum #

Answer 21

The atomic orbitals are first described by the principal quantum number (n), which describes how far the electron is from the nucleus. n = 0, 1, 2, 3 The higher the value of n, the larger the orbital. The higher the value of n, the higher the potential energy.

Question 22

quantum mechanics

Answer 22

Scientists studied hydrogen’s spectrum and found a pattern that enabled them to develop a model to predict the probability of finding an electron at any location: can be expressed graphically by atomic orbitals

Question 23

ionization energy

Answer 23

energy required to move an electron from an atom in a gaseous state

Question 24

non-metal

Answer 24

upper right side/periodic. diving line b/w metals and nonmetals. solid @ room temp. other are gaseous. tned to be poor conductors of heat and electricity, tend to GAIN electrons in chemical changes

Question 25

orbital

Answer 25

• can contain up to two electrons and has a particular shape and orientation. e.g. is the z-aligned orbital in the p subshell in the second shell.

Question 26

what does Z equal in the Zeff equation

Answer 26

Z = the nuclear charge = the number of protons

Question 27

pauli exclusion principle

Answer 27

Atoms other than Hydrogen have more than one electron in them. Just like bowling balls on a hill, electrons all want to go to the lowest energy level (n=1, s subshell). However, just as people need space, electrons need their own space too! It turns out that at most two electrons can occupy one atomic orbital. Furthermore, the two electrons must have opposite electron spins (spin up ↑ and spin down ↓).

Question 28

how do you find the number of angular nodes?. Define each variable

Answer 28

l

l= angular momentum QN

Question 29

what 2 factors does the atomic radius depend on

Answer 29

The valence orbital, The larger the value of n, the larger the atom Zeff, The larger Zeff, the smaller the atom

Question 30

halogens

Answer 30

group 7. most familiar is chlorine, very reactive nonmetals

Question 31

how do you find the total number of nodes? explain each variable

Answer 31

n-1 n= principle quantum number

Question 32

noble gases

Answer 32

group 8. chemically inert, full valence electrons

Question 33

ionic radius

Answer 33

For a specific element, the radius decreases with increasing positive charge As you go down the periodic table, the ionic radius increases

Question 34

magnetic quantum #

Answer 34

The magnetic quantum number, ml, describes the spatial orientation. ml = -l, … , -1, 0, 1, … , l

Question 35

isoelectronic

Answer 35

radius decreases with increasing protons,(atomic number)/ positive charge

Question 36

emission spectrum

Answer 36

Spectrum assosiated with emission of electromagnetic radiation by elements or compunds

Question 37

alkaline earth metals

Answer 37

fairly reactive, not as reactive as alkali

Question 38

whats the principal QN symbol possible value, other name, and effects

Answer 38

symbol: n

possible values: 0,1,2,3,…

AKA: shell

Effects: orbital

Question 39

in effective nuclear charge, the properties of an atom are determiend by

Answer 39

The charge of the nucleus 2) The repulsion between electrons 3) The wave nature of the atomic orbitals

Question 40

ground state

Answer 40

state of atom/molecule in which electrons occupy the lowest possible energy orbitals available

Question 41

subshell

Answer 41

Subshell - a group of orbitals with particular properties like shape and angular momentum. Labelled s, p, d, f, g etc.

Question 42

hunds rule

Answer 42

energy orbital in a subshell is singly occupied w/ one electron any one orbital is doubly occupied. All electrons in singly occupied orbitals have same spin

Question 43

bonding atomic radius

Answer 43

The bonding atomic radius is defined as one-half of the distance between covalently bonded nuclei

Question 44

how do you find the number of radial nodes

Answer 44

n-1-L