Aromic Structure Flashcards

1
Q

Isotopes

A

Nuclei that have the same number of protons but different number of neutrons = same physical and chemical properties

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2
Q

Binding energy

A

Energy needed to bind together the nucleus of atoms

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3
Q

Nuclear decay

A

The nucleus prior to nuclear decay is called the parent and the nucleus formed as a results of nuclear decay is called the daughter nucleus

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4
Q

Alpha particles

A

High velocity He atoms that are enmities by alpha decay, which steal two electrons and become helium

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5
Q

Beta particle

A

High velocity electrons

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6
Q

Alpha

A

Daughter has mass number 4 less than parent, atom mic number 2 less than parent

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7
Q

Beta

A

Daughter will always be a different element but will have the same mass number as parent

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8
Q

Gamma

A

Daughter is identical to parent, except it has less energy

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9
Q

First order decay

A

The probability that a nucleus will decay in a given time is constant and independent of the surrounding of the nucleus

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10
Q

Half life Equation

A
n = noe^-kt 
t(1/2) = ln2/k
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11
Q

Principal quantum number (n)

A

Describes the distinct energy levels or shells of the electron that orbits the nucleus; # of e- = 2n^2

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12
Q

Secondary quantum number (l)

A

Refers to the subshell with in each energy level; l=0:uses s, l=1:uses p, l=2:uses d, l=3:uses f

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13
Q

Magnetic quantum number (ml)

A

Refers to the electron orbitals with each subshell; every s has 1 orbital, every p has 3 orbitals, every d has 5 orbitals, every f has 7 orbitals

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14
Q

Magnetic quantum number possibilities

A

s: 1 ml =0
p: 3 ml = -1,0,+1
d: 5 ml = -2,-1,0,+1,+2
f: 7 ml = -3,-2,-1,0,+1,+2,+3

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15
Q

Spin quantum number (ms)

A

Can either be +(1/2) or -(1/2), for up or down arrows respectively, follows Pauli exclusion principle

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16
Q

Pauli exclusion principle

A

States that no two electrons in the same atom may ever have completely identical quantum numbers (n, l, ml, ms)

17
Q

Aufbau principle

A

To find the correct ground state electron configuration of an atom, always completely fill all lower energy orbitals before filling any higher energy orbital

18
Q

Hund’s rule

A

When partially filling degenerate orbitals of p, d, and f subshell a, always put on electron in each orbital before pairing them up; unpaired e- are orient so that their magnetic spins are all aligned

19
Q

Violation of Aufbau principle

A

Extra stabilization is realized when an atom has a half filled or completely filled d orbital; Cr and Cu promote the 4s electron to the higher 3D subshell

20
Q

Transition metal ions

A

Unlike other elements, transition metals always lose all their s electrons before losing any d electrons