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business managment > Science > Flashcards

Science Flashcards

1
Q

Electron configuration Na

A

1s2 2s2 2s6 3s1

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2
Q

Electron configuration Br

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

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3
Q

electron configuration neptunium

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 5p6 6s2

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4
Q

how many protons and neutrons in Sulfur

A

16, 16

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5
Q

protons and neutrons in phosphorus

A

15, 16

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6
Q

What’s the relative atomic mass C

A

12.0

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7
Q

Which of the subatomic particles does not have ‘mass’ relative to the other subatomic particles

A

Electrons

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8
Q

What is a ‘group’ on the periodic table?

A

top to bottom and measure how many electrons are in the valence shell

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9
Q

What are periods

A

left to right and tell us how many shells are in each element

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10
Q

Which element is in Group 2, Period 3?

A

Magnesium

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11
Q

What is the difference between relative atomic mass and mass number

A

Mass number is protons plus neutrons
relitive atomic mass is the average mass of all the isotopes

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12
Q

atomic radius … down a group

A

increases

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13
Q

atomic radius … across a period

A

Decreases 3

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14
Q

what is the unit used to measure an atom

A

AMU - atomic mass unit

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15
Q

How many electrons can the S subshell have

A

2

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16
Q

P

A

6

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17
Q

D

A

10

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18
Q

F

A

14

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19
Q

metals … electrons

A

lose

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20
Q

non-metals … electrons

A

gain

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21
Q

non metals form

A

negatively charged ions

22
Q

metals form

A

positively charged ions

23
Q

what are ions

A

atoms that have an electrical charge

24
Q

what is the core charge

A

it is a measure of the positive charge protons in the nucleus experienced by the valence electrons

25
Q

how is core charge calculated

A

protons - nonvalent electrons

26
Q

what is boron core charge

A

5-2= 3+

27
Q

what does a bigger core charge mean

A

electrons are more attracted

28
Q

smaller core chare means easier to

A

take electrons

29
Q

bigger core charge the smaller/bigger it is

A

smaller because closer together

30
Q

core charge of nitrogen

A

7-2 = 5+

31
Q

core charge of phosphorus

A

15-10 +5+

32
Q

what is the shielding effect

A

the ‘blocking’ ‘counseling’ of the nucleus by the inner shell electrons

33
Q

core charge more shells =

A

more electron shielding

34
Q

even though P and N have the same charge … valence shells are more shielded

A

P because there are more shells

35
Q

shielding increases going … but doesn’t change

A

down a group across a period

36
Q

core charge … going across a ….

A

increases period but doesn’t change going down a group

37
Q

atomic radius is the distance between

A

nucleus and outer most occupied electron shell

38
Q

atomic radius … as more shells are added (down a group)

A

increases

39
Q

atomic radius … across a period

A

decreases

40
Q

why does the atomic radius decrease across a period

A

the shells are held more tightly to the nucleus

41
Q

what is electronegativity

A

a measure of an element’s ability to pull towards itself in a bond

42
Q

greater core charge =

A

greater electronegativity

43
Q

the more shielding =

A

less electronegativity

44
Q

electronegativity … down a group

A

decreases

44
Q

the more positive charge a species has the … its electronegitivity

A

higher

45
Q

electronegativity … across a period

A

increases

46
Q

what is first ionization energy

A

the energy required to remove a single electron from the valence shell of an atom

47
Q

as core charge increases electrons are attracted more/less strongly to the nucleus

A

more

48
Q

the shielding effect increases electrons are attracted…

A

less

49
Q

ionization energy … across a period

A

increases

50
Q

core charge increases = ionization energy

A

increases

51
Q

shielding effect increases = ionization energy

A

decreases

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