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Chemestry 1h > Electrons Abd Such > Flashcards

Electrons Abd Such Flashcards

0
Q

Electro magnetic spectrum

A

Shorter wavelength higher frequency

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1
Q

Electron

A

Emission of light

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2
Q

Bohr models

A 
Rings
2
8
18
32
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3
Q

Ground state

A

Lowest state of energy an electron can be at

Most stable

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4
Q

Excited state

A

State higher than ground state

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5
Q

What does n cloud describe

A

Energy levels

Larger value of n=more distance from nucleus higher the energy

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6
Q

Quantum number L describes

A

Types of clouds

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7
Q

Four types of l clouds

A

S
P
D
F

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8
Q

What four elements have exceptions in electron filling

A

Cu
Cr
Ag
Au

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9
Q

Pauli exclusion principle

A

Max of 2 electrons per orbital

Must have different spin

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10
Q

Aufbau principle

A

Electrons occupy lowest energy orbitals available

And orbital can hold 2 electrons

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11
Q

Hunds rule

A

Orbitals of equal energy occupied by 1 electron before 2 electrons
All electrons singly occupied must have same spin

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12
Q

Paramagnetic

A

Attracted to magnets

Contains 1 or more in paired electrons

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13
Q

Diamagnetic

A

Not attracted to magnets because all electrons are paired

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14
Q

Newlands

A

First person to use periodic table
16 elements
Organized them by increasing atomic mass
Made law of octaves

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15
Q

Law of octaves

A

Chemical and physical properties repeated with 8th element

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16
Q

Medelev

A

63 elements

Left gaps

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17
Q

Mosley

A

Rearranged table
Increasing atomic number
Made periodic law

18
Q

Periodic law

A

Chemical and physical properties of elements periodic functions of their atomic numbers

19
Q

Alkali metals

A

React with water to produce basic solutions

First group on the left

20
Q

Alkaline earth metals

A

Less reactive than alkali

2nd group to the left

21
Q

Lanthanides

A

Color tv

1st group on f block

22
Q

Actinides

A

Radioactive

2nd group on f block

23
Q

Transition metals

A

D block

Solutions often colored

24
Q

Halogens

A

Salt formers

2 group from right

25
Q

Noble gases

A

Very stable
Filled outer electron orbitals
1st group to the right

26
Q

Metals

A

Conductivity
Shiny
Malleable
Ductile

27
Q

Alloy

A

Metal+nonmetal

Stainless steel Fe+cr

28
Q

Non metals

A

To the right of metalloids

29
Q

Metalloids

A

Semi conductors
Staircase on periodic table
B, si, ge, as, sb, te

30
Q

Atomic radius

A

Half he distance between nuclei of adjacent atoms bonded to each other

31
Q

Vander waals radius

A

Half the distance between nuclei of adjacent atoms not bonded to each other

32
Q

Difference between atomic bond radius and vander waals radius

A

Atomic bond radius smaller than vander waals radius

33
Q

As you move down a group atomic radius…

A

Increases

1 energy level is added down each period

34
Q

Electron sheik ding effect

A

Electrons in inner energy levels shield outer electrons from full nuclear charge

35
Q

As you move across a period atomic radius

A

Decreases
Increasing nuclear charge
Electrons: same energy level

36
Q

Across a period

A

Protons added= increased positive charge

Electrons added=same energy level

37
Q

Ion

A

Atom with an electrical charge

38
Q

Positive ion

A

Loses and electron

39
Q

Negative ion

A

Gains an electron

40
Q

Ionization energy

A

Energy needed to remove outer electron from and atom

41
Q

As you love across a period ionization energy

A

Increases

Electrons held more tightly to nucleus

42
Q

As you go down a group ionization energy

A

Decreases

Electrons held less tightly to nucleus

43
Q

Electron affinity

A

Energy emitted upon addition of electron to atom

Chemestry 1h (9 decks)

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