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Chemistry > Chapter 5-Electron Configuration > Flashcards

Chapter 5-Electron Configuration Flashcards

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1
Q

What can be used to determine electron arrangement in an atom?

A

set of 3 rules: aufbau principle, Pauli exclusion principle, Hund’s rule

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2
Q

All atoms can be described with orbitals similar to…

A

Hydrogen’s orbitals

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3
Q

electron configuration

A

arrangement of e’s in an atom

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4
Q

E’s assume the arrangement that gives the atom the _____ energy possible

A

lowest

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5
Q

ground state e configuration

A

most stable, lowest energy arrangement of e’s

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6
Q

aufbau principle

A

each e occupies lowest energy orbital available

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7
Q

aufbau diagram

A

shows sequence of atomic orbitals from lowest to highest energy

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8
Q

aufbau: all orbitals related to an energy sublevel are of…

A

equal energy

ex. all three 2p orbitals are of equal energy

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9
Q

aufbau: in a multi-e atom, the energy sublevels w/in a principal energy level have…

A

different energies

ex. the three 2p orbitals are of higher energy than the 2s orbital

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10
Q

aufbau: orbitals related to energy sublevels w/in one principal energy level can ____ orbitals related to energy sublevels w/in another principal level

A

overlap

ex. 4s sublevel has lower energy than 3d sublevel

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11
Q

e’s in orbitals are represented by ____ in _____

A

arrows…boxes

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12
Q

empty box represents

A

unoccupied orbital

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13
Q

pauli exclusion principle

A

max of 2 e’s can occupy a single atomic orbital, but only if they have opposite spins

by Wolfgang Pauli after observing excited atoms

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14
Q

max number of e’s related to each principal energy level is…

A

2n^2

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15
Q

Hund’s rule

A

single e’s w/ same spin must occupy each equal-energy orbital before additional e’s w/ opposite spins can occupy the same orbitals

ex. ^ ^ ^, then ^v ^ ^

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16
Q

ways to represent e configuration

A

orbital diagrams

electron configuration notation

17
Q

orbital diagram

A

arrows in boxes

each box labeled with principal quantum # and sublevel associated w/ orbital

18
Q

electron configuration notation

A

1s^2 2s^2…

doesn’t usually show the orbital distributions of e’s related to a sublevel

19
Q

noble gas notation

A

shortcut e configuration w/ noble gas
has ns^2 and np^6 full

[Ne]3s^2

20
Q

noble gases

A

elements in last column of periodic table
8 e’s in outermost orbital
stable

21
Q

exceptions to Aufbau Rule

A

chromium: [Ar]4s1,3d5
copper: [Ar]4s1,3d10

to be more stable, draw box diagram to see (look at video)

22
Q

valence e’s

A

e’s in outermost orbitals

OCCUPY THE S AND P OF THE SAME HIGHEST ENERGY LEVEL

23
Q

what do valence e’s determine?

A

chemical properties of an element

24
Q

why do scientists only show valence e’s in e-dot structures?

A

since these e’s are involved in forming chemical bonds

25
Q

electron dot structure

A

element’s symbol w/ dots around it representing the valence e’s

26
Q

who devised the electron dot structure method?

A

G.N. Lewis (American chemist)

27
Q

Aufbau rule is also called the what?

A

diagonal rule

28
Q

Which rule supports the box diagram?

A

Hund’s rule

29
Q

isoletric

A

when atoms have same e configuration

30
Q

How do you determine an atom’s charge?

A

write out e configuration and see if it would be easier to take in e’s or lose e’s

gain: (-) charge
lose: (+) charge

31
Q

How to write e configuration of atoms with a charge

A

ex. Pd^(+2)
[Kr]5s2,4d8 –> [Kr]4d8
lose 2 e’s (take from outermost orbital w/ highest
energy level)

32
Q

diamagnetic

A

paired e’s

^v ^v

33
Q

paramagnetic

A

unpaired e’s aligned w/ a magnetic field

34
Q

farromagnetic

A

unpaired e’s that remain aligned when no magnetic field exists
*Fe the only element

35
Q

Periodic Table (where are the sublevels located?)

A

(look at skitch)

36
Q

positive ions are ____ and negative ions are ____

A

metal

non metals

37
Q

In which principal energy level do the different sublevels begin to overlap?

A

n=4

the d’s

38
Q

what does each sublevel look like?

A

Spherical: sphere
Principal: dumbbell
Diffuse: donut shape
Fundamental: multiple

39
Q

How many e’s can each sublevel hold?

A

s: 2
p: 6
d: 10
f: 14

Chemistry (5 decks)

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