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Chemistry > Atoms and the Periodic Table > Flashcards

Atoms and the Periodic Table Flashcards

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1
Q

What does an atom consist of?

A

Nucleus, protons, neutrons, shells

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2
Q

Define nucleus

A

The heavy core at the centre of an atom that contains neutrons and protons

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3
Q

What are the different charges?

A

Protons +
Neutrons - neutral
Electrons -

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4
Q

qualities of Electrons

A

Spin around the space surrounding the nucleus
Neg charged
Attracted to positive nucleus

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5
Q

qualities of Protons

A

Are in the nucleus

The no. of protons = no. of electrons

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6
Q

qualities of Neutrons

A

Are neutral

Heavier than protons and 1800 the size of electrons

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7
Q

What are elements?

A

Building blocks of all substances

Each element is made of atoms

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8
Q

how is the periodic table oragnised?

A

Vertical groups

Horizontal periods

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9
Q

what does the atomic number determine

A

= protons and electrons

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10
Q

what is the mass number made of

A

is protons + neutrons

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11
Q

define Compounds

A

A substance that is made of 2 or more elements bonded together

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12
Q

What are the 5 groups on the periodic table?

A 
Alkali metals
Alkaline earths
Halogens
Noble gases
Transition metals
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13
Q

what are the Periods

A

the horizontal rows

the period number is the same number of electron shells it has

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14
Q

what are the Groups

A

the vertical columns
they have the same properties
the last digit of the group number is the number of electrons in the outer shell

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15
Q

Alkali metal

A

Form cations of +1
Really reactive
Group 1

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16
Q

Alkaline Earths

A

Group 2
Similar to group 1
Form a +2 cation

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17
Q

halogens

A

Group 17
Form anions with -1
mean salt producing

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18
Q

Noble gases

A

Group 18
Inert gases
stable

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19
Q

Transition metals

A

group 3-12
hard, high melting/boiling points
useful/valuable metals

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20
Q

Orbitals

A

Are volumes of space where electrons are most likely to be found

21
Q

Subshells

A

are a way of grouping similar orbitals

22
Q

Shells

A

groups orbitals with similar energy

23
Q

how many orbitals in each subshell

A

s=1
p=3
d=5
f=7

24
Q

What is the orbital filling rule

A

Aufbau’s

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 4f, 5d, 5f

25
Q

What are the different bonding types?

A

metallic, ionic, covalent

26
Q

metallic bonding

A

between 2 metals

has cations and a sea of delocalized electrons

27
Q

ionic bonding

A

between metal and non-metal

cations and anions line up next to the opposite to form a lattice

28
Q

covalent bonding

A

between nonmetals

non metals bonding

29
Q

Ions

A

Are atoms that have become charged because they have gained or lost electrons

30
Q

Cation

A

a positively charged ion
have more protons than electrons
form when metals lose their outer shell electrons

31
Q

Anion

A

negatively charged
more electrons
form when non-metals gain electrons

32
Q

What are atoms?

A

are the particles that make all the substances up in the universe

33
Q

smallest particle that everything can be divided to

A

atom

34
Q

where are electrons most likely to be found?

A

electron clouds

35
Q

every atom of a given element has the same number of what?

A

protons

36
Q

an isotope always has

A

the same number of protons

37
Q

atoms to the right of the zigzag in the periodic table are

A

nonmetal

38
Q

what are the zigzag atoms

A

metalloids

39
Q

what is something with the same number of protons but different number of electrons called

A

ion

40
Q

who discovered the electron

A

j.j thompson 1897

41
Q

what are excited electrons

A

when they shell jump, it requires energy to jump up and then when they return to ground state their excess energy releases as light

42
Q

lanthanides

A

a special block of metallic elements with atomic numbers 57-71

43
Q

actinides

A

a special block of metallic elements with atomic numbers 89-103

44
Q

ground state

A

the lowest energy arrangement of an atom’s electrons in energy levels

45
Q

if an element has an electron configuration of 2,6 or 1s2, 2s2, 2p4 what charge would it form as an ion

A

2, 6 < 6 need 2 electrons which are neg

so -2

46
Q

metallic bonding looks like…

A

cations surrounded by a bunch of delocalised electrons

47
Q

ionic bonding looks like…

A

in a lattice of the cations and anions lining up next to one another

48
Q

covalent bonding looks like…

A

the molecules share electrons

Chemistry (5 decks)

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