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chemistryyyy > Ch301 Unit 1 Test Ep9-11 > Flashcards

Ch301 Unit 1 Test Ep9-11 Flashcards

1
Q

Pauli Exclusion Principle

A

No 2 e- in an atom have the same 4 quantum numbers

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2
Q

Aufbau principle

A

Electrons fill from lowest E to highest E orbitals

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3
Q

Hunds Rule

A

Electrons fill degenerate orbitals singly before pairing up

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4
Q

Diamagnetic

A

An atom with all paired electrons

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5
Q

What type of element in the first group

A

Alkali metals

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6
Q

What type of metal is in the second group?

A

Alkali earth metal

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7
Q

What type of metal is found in d block?

A

Transition metals

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8
Q

What type of element is found in group 7

A

Halogens

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9
Q

What type of lament is found in group 8 of the periodic table

A

Noble gases

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10
Q

Radial distribution

A

The closer the negative electron is the positive nucleus, the stronger the electrostatic attraction, and the lower the E

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11
Q

Atoms achieve greater stability when

A

Their subshells are completely full or half full

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12
Q

Anytime you do econfig of ions in d orbital what needs to happen

A

You need to reorder the numbers in number order then remove e- from the right to the left

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13
Q

Do all e- in atom feel same strength of attraction to nucleus?

A

No the e- in a lower E level feel a stronger attraction to the nucleus

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14
Q

As you move across a row what happens to Zeff

A

Gets larger cuz more VE

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15
Q

How do they measure atomic radius

A

Distance between 2 nucleus when they next to each other because you can’t measure atomic cloud because it isn’t strictly defined

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16
Q

Atomic radius trends

A

Decreases L to R
Increases down

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17
Q

Positive ions are bigger or smaller than regular

A

Smaller

18
Q

Negative ions are bigger or smaller than regular

A

Bigger

19
Q

what is IE

A

The amount of E required to remove the first e- from a neutral atom in the gaseous state

20
Q

IE vs work function

A

IE is the removal of an electron from a single gas phase atom vs the electron from a single gas phase atom

21
Q

Equations for first IE

A

X(g) + e- -> O-(g)

22
Q

EA

A

The change in E when an e- is added to a gaseous atom to form an anion

23
Q

EA values are positive

A

Endothermic heat being added

24
Q

EA are negative

A

Exothermic
Heat being released

25
Q

Why does EA increase

A

Because of increased nuclear attraction

26
Q

What is the IE trend based off

A

Nuclear charge and fully filled/half filled subshells

27
Q

What trend is EA based off

A

It has no consistent trend but when comparing two neighboring atoms you can look at half or fully filled subshells

28
Q

What is n1 in the Rydberg equation

A

The one that the atom drops to, the lower n

29
Q

What is ground energyelevel

A

N=1

30
Q

What is n =1 in Rydberg equation

A

N=1 is the final level the e- is on

31
Q

Why does high EA mean?

A

More negative

32
Q

What does EA mean?

A

More electronegative, higher tendency to take electrons

33
Q

What happens to the wavelength the larger the size of the item?

A

The smaller the wavelength

34
Q

Stoich

What’s conversion from grams to atoms with the molecule H2O

A

Grams to moles to molecules to atoms

35
Q

Conversion from atoms to grams with molecule H2O

Stoic

A

Grams to moles to molecules to atoms

36
Q

What unit is avigadros number for?

A

Molecules

37
Q

When doing stoich ions are the same as +

A

Molecules

38
Q

Completely removing an electron from an atom entirely means?

A

Moving it to the infinity energy level

39
Q

What is infinity squared!

A

0

40
Q

What does ionizing mean

A

Completely removing an e-

41
Q

When dealing with completely removing an e- or ionizing an e-(same thing) which number comes first in the rydberg formula for n1

A

The real number, then n2 = infinity

42
Q

Balmer series

A

Portion of the emission spectrum of H that represents electron transitions from energy levels E>2 to n=2

chemistryyyy (40 decks)

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