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IMAT > The Periodic Table > Flashcards

The Periodic Table Flashcards

1
Q

Hydrogen

A

H
first group and period
atomic number- 1
mass number- 1
NON-METAL

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2
Q

Lithium

A

Li
first group & second period
atomic number- 3
mass number- 7

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3
Q

Sodium

A

Na
first group & third period
atomic number- 11
mass number- 23

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4
Q

Potassium

A

K
first group & fourth period
atomic number- 19
mass number- 39

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5
Q

Beryllium

A

Be
second group & second period
atomic number- 4
mass number- 9

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6
Q

Magnesium

A

Mg
second group & third period
atomic number- 12
mass number-24

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7
Q

Calcium

A

Ca
second group & fourth period
atomic number- 20
mass number- 40

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8
Q

Barium

A

Ba
second group & sixth period
atomic number-56
mass number- 137

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9
Q

Radium

A

Ra
second group & seventh period
atomic number- 88
mass number- 226

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10
Q

Boron

A

B
group- 13 (3)
period- 2
atomic number- 5
mass number- 11
METALLOIDS

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11
Q

Carbon

A

C
group- 14 (4)
period- 2
atomic number- 6
mass number- 12

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12
Q

Nitrogen

A

N
group- 15 (5)
period- 2
atomic number- 7
mass number- 14
very electronegative

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13
Q

Oxygen

A

O
group- 16 (6)
period- 2
atomic number- 8
mass number- 16
very electronegative

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14
Q

Fluorine

A

F
group- 17 (7)
period- 2
atomic number- 9
mass number- 19
very electronegative

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15
Q

Aluminium

A

Al
group- 13 (3)
period- 3
atomic number- 13
mass number- 27

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16
Q

Silicon

A

Si
group- 14 (4)
period- 3
atomic number- 14
mass number- 28
METALOIDS

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17
Q

Phosphorus

A

P
group- 15 (5)
period- 3
atomic number- 15
mass number- 31

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18
Q

Sulfur

A

S
group- 16 (6)
period- 3
atomic number- 16
mass number- 32

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19
Q

Chlorine

A

Cl
group- 17 (7)
period- 3
atomic number- 17
mass number- 35.45
very electronegative

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20
Q

Bromine

A

Br
group- 17 (7)
period- 4
atomic number- 35
mass number- 80

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21
Q

Iodine

A

I
group- 17 (7)
period- 5
atomic number- 53
mass number- 127

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22
Q

Helium

A

He
group- 18 (8)
period- 1
atomic number- 2
mass number- 4

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23
Q

Neon

A

Ne
group- 18 (8)
period- 2
atomic number- 10
mass number- 20

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24
Q

Aragon

A

Ar
group- 18 (8)
period- 3
atomic number- 18
mass number- 40

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25
Alkali Metals
the first group have only one electron in their valance shell, therefore have the same chemical properties Cations: 1+ low density and low melting point react with water fast in their elemental state.
26
Alkaline Earth Metals
the second group have two electrons in their valance shell Cations: 2+ low melting and boiling point
27
Halogens
group number 7 have 7 electrons in their valence shell Anion: 1- usually found in the form of a diatomic molecule Are found in our bodies in small amounts- large quantities are toxic!!
28
Noble Gases
group 8 have 8 electrons in their valence shell very stable do not form ions - odorless -colorless
29
Why Helium (He) is Special?
he has only 2 electrons in their valence shell, unlike the rest of the noble gases - still stable
30
Why Hydrogen (H) is Special?
belongs to group 1 only because it's atomic structure. but has chemical properties of non metal, hence he is in group 1 but not part of the alkali metals family.
31
Transition Metals
found in the d block of the periodic table Cations!! can form more than one kind of cation to become stable: copper can form (1+) and (2+) ions. properties of metals high boiling and melting point (exept mercury) high density
32
What are the metals properties?
- solid at room temperature - high density - conduct electricty and heat well - hard and rigid - distinctive luster - cations
33
What are the properties of non metal?
- low melting and boiling point - poor conducors of electricity and heat - brittle - may be colorful, but no luster - anions - gaseos in room temp (most)
34
what is special about mercury?
unlike the rest of the metals, he is liquid in room temp.
35
what is so special about bromine?
unlike the rest of the non- metals, he is liquid in room temp.
36
What are alloys?
mixture of metals or metal with non metal, harder' stronger and less reactive than pure metals
37
Bronze
Alloy- combination of tin (Sn) and copper (Cu)
38
Steel
Alloy- combination of iron (Fe) and carbon (c)
39
What is the effect of the size of the nuclear charge on the electrons in the atom's orbitals?
atomic number increasing ---> more positive protons in the nucleus---> larger positive charge---> stronger attraction between the electrons to the nucleus ---> more energy is required to remove the electrons (harder)
40
What is the effect of the number of electron shells on the electrons in the atom's orbitals?
more sells ---> distance from the nucleus is bigger ---> less energy is needed to remove electrons (easier) + effective nuclear charge is smaller
41
Chemical reactivity
the tendency to gain or lose electrons. metals prefer to lose' while non metals prefer to gain.
42
Why the center of the periodic table is less reactive than the sides?
it is easier to gain or lose one electron rather than two or three. the closer to full valence shell, more reactive it is
43
Atomic Radius
atomic size- the distance from the nucleus to the valence electrons. the larger the atomic radius, the larger the atoms.
44
Why the atomic radius decreases across a period?
no increase in energy level + increase i the nuclear charge ---> the attraction between the nucleus and the electrons increases and the distance between them decreases
45
why the atomic radius increasing down a group?
the number of electron shells increases, more energy leve more distance. there is greater nuclear charge, but the inner electrons sielding is greater as well
46
ionic vs. atomic radius
cations radius is smaller than their atomic radius anions radius is larger than their atomic radius.
47
What is shielding?
when the valence electron feels less of the positive nuclear charge, because the inner electrons create repulsive forces, so the valence electrons feel smaller positive reaction
48
why the electrical conductivity increasing across the metals of the same period?
increasing number of delocalized electron in the metalic lattice, in the non metals of the same perios it will decrease
49
why is the melting point increasing across the metals of the same period?
the structure of the metalic lattice and increase of delocalized electrons non metals create covalent bonds, which are weaker and have lower melting point.
50
Electronegativity
the tendency to attract electrons twowrds itself (does'nt creat anions), usually in chemical bonds
51
why does the electronegtivity increases across a period?
the effective nuclear charge is increasing, and the nucleus is more liklely to attract + radius is smaller, causing greater attraction
52
why does the electronegtivity decreases down a group?
shielding effect is larger, while the effective nuclear charge is the same + bigger radius, decreases attraction
53
what are the most electronegative elements, by order?
F > O > Cl > N
54
what are the least electronegative elements?
carbon and hydrogen
55
ionization energy
the amount of energy required to remove a single electron from the valence shell of an atom, forming a cation.
56
first ionization energy
the amount of energy required to remove the first electron from each atom in one mole of elements in their gaseus state.
57
why is it requires more energy to remove electrons after the first one?
the removal of electrons creats positive charge, which increases as more electrons are removed. when the positive charge increases, the attraction to the remaining electrons also increases, and more energy is required to remove the electrons.
58
second ionization energy
the amount of energy required to remove the second electron from each atom in one mole of elements in their gaseus state.
59
Effective Nuclear Charge
the positive charge felt by the higher-shell electrons
60
What affects the effective nuclear charge
- size of nucleus (number of protons) - number of inner electrons (shielding)
61
why does the effective nuclear charge incresases across a period?
more protons in the nucleus, while the numner of inner electrons (energy levels) remain the same.
62
why is'nt there any change in the effective nuclear charge down a group?
the number of electrons added is equal to the increase in the number of positive electrons the actual attraction between protons and electrons decreases, due to the increasing distance
63
Electron Affinity
the amount of energy released, when an electron uss added to an atom in its gaseus state- forming an anion
64
How can we calculate effective charge?
Z(eff) = Z(#p) - S(#e shielding)

IMAT (32 decks)

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