Exam 1 (chapters 1-4) Flashcards by mj Unknown

10^6

mega- (M)

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10^-6

micro- (µ)

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10^-9

nano- (n)

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Aufbau Principle

e- fills the lowest energy level first

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3*10^8 m/s

Speed of light

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Hund’s Rule

-e filled in the same energy level in 1 orbital at a time and is oriented in the same direction

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no two e- in an orbital can have the same spin

Pauli Exclusion Principle

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the ion with the most protons is the smallest b/c there are more protons in the nucleus to pull fewer e- in the shells

for ions of an isoelectric series:

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How can you tell if an element is in an excited state from the electron configuration?

subshells that are not the last sub shell are not filled

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ℓ =0

Sub-shell s
-spherical

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ℓ=1

sub-shell p
3 orbitals
dumbbell shape

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ℓ=2

Sub-shell d
5 orbitals
cloverleaf shaped

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ℓ=3

Sub-shell f
7 orbitals

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Cr electron configuration

[Ar]4s^1 3d^5

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(2 *ℓ)+1

number of orbital or _ in a configuration

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Cu electron configuration

[Ar] 4s^1 3d^10

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Electron affinity (EA)

The energy change associated with the addition of an electron to a gaseous atom

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energy absorbed during the gain of an e-

EA is endothermic

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energy is released during the gain of an e-

EA is exothermic

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an atom is ionized when

an e- is leaving an atom; n(final)=∞

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attractive interactions are

negative

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repulsive interactions are

positive

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atoms of the same element with different neutrons

isotopes

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mechanical kinetic energy

-moving mass
-mechanical pot. energy
-stored mass in a place where a force acts

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electrical kinetic energy

-moving charge -electrostatic pot. energy b/c or the interaction of charged particles

light kinetic energy

-moving photons -chemical pot. energy -stored in bonds

heat enters a system

heat leaves a system

-q

work is done on a system

work is done by the system

-w

state function

a function that depends only on the initial and final states of a system, not the path in between. -represented by uppercase letters, P, V, H, T

electrostatic energy

proportional to the magnitude of the charges inverse to the distance between particles

enthalpy

heat transferred at a constant pressure

exothermic process

when energy (often as heat) leaves a system into the surroundings

endothermic process

energy (as heat) is added to a system

hc/λ

E(photon)=

Gamma ray wavelength range

<10^-8

UV and visible wavelength range

10^-8 to 10^-6

infrared wavelength range

10^-6 to 10^-4

microwave wavelength range

10^-4 to 10^-1

radio wavelength range

10^0 to 10^4

black body radiaiton

radiation emitted by an object

when light is reflected or transmitted...

the complementary color is absorbed

transmitted light

is not absorbed, passes through

when interacting with matter, gamma rays, x rays, UV rays...

-ionize atoms and molecules -break chemical bonds

when visible spectrum rays interact with matter (electronic transitions)

e- is promoted to higher energy

when infrared rays interact w matter

increased amplitude of vibrations (KE goes up)

microwave interactions with matter

rotations increase

radio waves...

flip nuclear spin

lowest energy is when

closest to p+ (ground state)

electron transition causes

e- moves from one allowed energy state to another e- changes energy levels emitting/absorbing photons

principle quantum number (n)

-info on orbital size -defines what shell e- is in info on orbital energy

quantum number ℓ

determines shape

magnetic quantum number (mℓ)

-describes orientation of orbital in 3D space - ranges from -ℓ to ℓ

node

no electrons n-1=nodes

core shielding

- inner e- shield valence e- from nucleus - outer e- experience less Ze and have a weak attraction - outer e- have less energy

atomic radius

increases down a group decreases across a period

ionization energy

energy needed to remove e- in gaseous state always positive increases across a period decreases down a group

Zeff for valence e-

increases down a group and across a period

EA is more negitive

across a period

size of ion relative to parent atom

anion>parent>cation

isoelectic series

group of atoms or ions that have the same number of e- (same ground state configuration)

effective nuclear charge (Zeff)

net positive charge experienced by valence e-

when valence e- are further from the nucleus

more reactive

metallic character and reactivity increase

as ionization energy decreases

IE=

energy needed to form a positive ion

E(g) --> (E+) + (e-)

ionization energy representation

electron affinity representation

E(g) + (e-) --> E(g)-

p block elements, nonmetals

elements that have ionization energies > 1000

metals s,d,f block elements

elements that IE<1000

potential energy

-stored energy - not a state function (path matters)

1000J

1KJ

Planck's Constant

6.63*10^-34 m^2kg/s

Avogadro's Number

6.02*10^23

Moles to grams conversion

# of moles * molar mass

Exam 1 (chapters 1-4) Flashcards

(75 cards)