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Chemistry 9 > Chapter 2 > Flashcards

Chapter 2 Flashcards

Atom Structure, Isotopes, Electron Shells, Energy Configuration, Periodic Table Structure

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1
Q

Amount and direction of periods of the periodic table?

A

7 horizontal rows

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2
Q

Amount and direction of groups of the periodic table?

A

18 vertical columns

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3
Q

What is the US division of the groups?

A

1A-8A and 1B-8B

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4
Q

What columns are the main group elements?

A

2 groups 1A-2A and 6 groups 3A-8A

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5
Q

What columns are the transitional metals?

A

What columns are the transitional metals?

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6
Q

What columns are the inner transition metals?

A

14 groups between 3B and 4B

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7
Q

How are elements divided in the periodic table?

A

Metals, nonmetals and metalloids

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8
Q

What side are the metals in the periodic table?

A

Left

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9
Q

What side are the nonmetals in the periodic table?’

A

Right

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10
Q

Where are the metalloids in the periodic table?

A

Along the solid line of the periodic table

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11
Q

What column are the Alkali metals?

A

Column 1A

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12
Q

What are the Alkali metals from top to bottom?

A

Li
Na
K
Rb
Cs

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13
Q

What column are the Alkaline Earth metals?

A

Column 1B

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14
Q

What are the Alkaline Earth metals from top to bottom?

A

Be
Mg
Ca
Sr
Ba

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15
Q

What column are the Halogens?

A

Column 7A

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16
Q

What are the Halogens from top to bottom?

A

F
Cl
Br
I
At

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17
Q

What column are the Noble Gasses?

A

Column 8A

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18
Q

What are the Noble Gasses from top to bottom?

A

He
Ne
Ar
Kr
Xe

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19
Q

What is the nucleus?

A

The dense core of the atom that holds protons and neutrons

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20
Q

The dense core of the atom that holds protons and neutrons

A

Empty space that holds electrons

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21
Q

What is the rule of particle charges?

A

Opposites attract, while equals repel

22
Q

What is an atomic number?

A

The number of protons in the nucleus

23
Q

What are isotopes?

A

Atoms of the same element that have a different number of neutrons

24
Q

What is the equation to find the mass number of an atom

A

Number of protons + number of electrons

25
Q

What is the atomic mass?

A

The weighted average of the masses of an element’s isotopes

26
Q

How to find the atomic mass?

A
  1. List each isotope, its mass in atomic mass units (amu), and its abundance in nature
  2. Multiply the isotopic abundance by the mass of each isotope
  3. add total amu’s together.
27
Q

What are shells?

A

The regions occupied by electrons around the nucleus that gives the nucleus a charge

28
Q

Formula to find max number of electrons a shell can hold

A

2n^(2) where n = shell number

29
Q

Are shells referred by letter or number?

A

Whole number

30
Q

What are subshells?

A

The energy sublevel inside each shell that electrons occupy

31
Q

Are subshells referred by letter or number?

A

Letter

32
Q

What are orbitals?

A

Regions inside subshell that an electron can likely be found

33
Q

Name each subshell with its orbitals and the amount of electrons it can hold

A

s: One orbital, Two electrons
p: Three orbitals, Six electrons
d: Five orbitals, Ten electrons
f: Seven orbitals, Fourteen electrons

34
Q

How many electrons can an orbital hold?

A

2

35
Q

What is the shape of an s orbital?

A

Spherical shape

36
Q

What is the shape of a p orbital?

A

Dumbbell shape

37
Q

First shell: Name subshells, orbitals and electrons

A

1s = 1 orbital: 2 electrons

2 electrons total

38
Q

Second shell: Name subshells, orbitals and electrons

A

2s = 1 orbital = 2 electrons
2p = 3 orbitals = 6 electrons

8 electrons total

39
Q

Third shell: Name subshells, orbitals and electrons

A

3s = 1 orbital: 2 electrons
3p = 3 orbitals: 6 electrons
3d = 5 orbitals: 10 electrons

Total electrons: 18

40
Q

Fourth shell: Name subshells, orbitals and electrons

A

4s = 1 orbital = 2 electrons
3p = 3 orbitals = 6 electrons
4d = 5 orbitals = 10 electrons
4f: 7 orbitals = 14 electrons

Total electrons: 32

41
Q

Fifth shell: Name subshells, orbitals and electrons

A

5s = 1 orbital = 2 electrons
5p = 3 orbitals = 6 electrons
5d = 5 orbitals = 10 electrons
5f: 7 orbitals = 14 electrons

Total electrons: 32

42
Q

Sixth shell: Name subshells, orbitals and electron

A

6s = 1 orbital = 2 electrons
6p = 3 orbitals = 6 electrons

Total electrons: 8

43
Q

Elements in the same column (group) have similar:

A

Electron configurations and chemical properties

44
Q

Elements in the same column (group) have the same:

A

number of valence electrons

45
Q

What are Electron Dot Symbols:?

A

Dots that represent valence electrons that are placed on the four sides of an element symbol

46
Q

Elements with 1-4 valence electrons use single/paired dots for electron dot symbols?

A

Single

47
Q

Elements with more than 4 valence electrons use single/paired dots for electron dot symbols?

A

Paired

48
Q

Does the size of atoms increase or decrease down a column? Why?

A

Increase, valence electrons farther from the nucleus

49
Q

Does the size of atoms increase or decrease across a row? Why?

A

Decrease, number of protons in nucleus increase, so valence electrons are brought closer

50
Q

What is ionization energy?

A

Energy needed to remove an electron from a neutral atom

51
Q

Do ionization energies increase or decrease down a column? Why?

A

Decrease, valence electrons get further from positive nucleus

52
Q

Do ionization energies increase or decrease down a column? Why?

A

Do ionization energies increase or decrease down a column? Why?

Chemistry 9 (6 decks)

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