Unit 3a Flashcards

1
Q

Group 1

A

Alkali metals

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2
Q

Group 2

A

Alkaline earth metals

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3
Q

Group 3-12

A

Transition metals

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4
Q

Group 13

A

Boron family

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5
Q

Group 14

A

Carbon family

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6
Q

Group 15

A

Nitrogen family

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7
Q

Group 16

A

Chalcogens

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8
Q

Group 17

A

Halogens

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9
Q

Group 18

A

Noble Gases

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10
Q

Valance electrons

A

electrons located in the outermost energy level of an atom furthest from the nucleus of the atom

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11
Q

How many valance electrons does Tin (Sn) have?

A

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12
Q

Why do atoms participate in bonding?

A

To become more stable

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13
Q

Cations

A

positive ions

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14
Q

Are cations bigger or smaller than its neutral atom?

A

smaller because it loses electrons

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15
Q

Anions

A

Negative ion

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16
Q

Are anions bigger or smaller than its neutral atom?

A

bigger because it gains electrons

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17
Q

Aufbau Principle

A

electrons enter orbitals of the lowest energy first

18
Q

Hund’s Rule

A

single electrons with the same spin must occupy each equal energy orbit before additional electrons with opposite spins can occupy the same orbitals

19
Q

Pauli Exclusion Principle

A

a maximum of 2 electrons cna occupy a single orbital (have to have opposite spins)

20
Q

What’s the electron configuration for Neon?

21
Q

What’s the orbital notation for Calcium (Ca)?

22
Q

What’s the octect rule?

A

tendency of atoms to prefer to have 8 electrons in the valance shell

23
Q

Electron configuration

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f

24
Q

What’s the five periodic table trends?

A

Ionization energy
electronegativity
atomic radius
ionic radius
metallic / non metallic character

25
principle quantum number symbol:
n
26
angular momentum quantum number symbol:
l
27
magnetic quantum number symbol:
ml
28
spin quantum number symbol:
ms
29
What is principal quantum number?
energy level n= 1-7 (period number)
30
What is angular momentum quantum number?
sublevel l= 0-3 s=0 , p=1 , d=2 , f=3
31
What is magnetic quantum number?
describes orbital orientation boxes (-2,-1,0,1,2)
32
What is spin quantum number?
1/2 or -1/2
33
Atomic radius
distance from the center of the atom to the outermost energy level of electrons Increases = top to bottom Decreases = left to right
34
Ionic radius
atomic radius for an ion Increases = top to bottom Decreases = left to right
35
Ionization energy
measure of energy needed to remove an electron from an atom Increases = left to right Decreases = top to bottom
36
Electronegativity
an atoms ability to attract an electron from another atom Decreases = top to bottom Increases = left to right
37
Metallic Character
Increases = top to bottom Decreases = left to right
38
What’s the 4 quantum numbers for Cobalt (Co)?
39
Draw the dot diagram for Sulfur (S)
40
Draw the Bohr diagram for Argon (Ar)