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Chemistry > 1 Periodic Table > Flashcards

1 Periodic Table Flashcards

1
Q

What was the need that arose?

A

To group the elements into families whose elements showed maximum rsemblance.

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2
Q 
Early chemists:
1. Basis of arranging
2 Method of arranging
3. Reason for discarding
4. Year
A
  1. On the basis of valency, metallic or non-metallic character.
  2. -
  3. Showed Variable Valency and dual character (metalloids).
  4. -
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3
Q 
Dobreiner:
1. Basis of arranging
2 Method of arranging
3. Reason for discarding
4. Year
A
  1. Atomic weights -> Increasing order
  2. Triads; At. weight of the middle element is average of the other two.
  3. It didnt hold true for all the elements.
  4. 1815
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4
Q 
Newland:
1. Basis of arranging
2 Method of arranging
3. Reason for discarding
4. Year
A
  1. Atomic weights -> Increasing order
  2. Series of eight; Property of every 8th element is the property of the 1st element.
  3. Didnt leave space for undiscovered elements.
  4. 1864
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5
Q 
Medeleef:
1. Basis of arranging
2 Method of arranging
3. Reason for discarding
4. Year
A
  1. Atomic weights -> Increasign order.
  2. In a table -> Mendeleef’s periodic table. Properties are periodic funcions of at. weight.
  3. Mehtod couldnt justify -> Certain elements, rare earth and isotopes.
  4. 1869
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6
Q 
Mosley:
1. Basis of arranging
2 Method of arranging
3. Reason for Adopting
4. Year
A
  1. Increased order of atomic numbers.
  2. In a table -> Modern periodic table. Properties are perioidc functions of atomic number.
  3. Method removes most of the defects of mendeleef.
  4. 1912
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7
Q

Which group in older notation has 3 groups?

A

VIII -> 8, 9 and 10

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8
Q

In older notation, 18th group is called?

A

0 group.

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9
Q

Why is atoms arranged in increasing order of atomic number?

A

Physical and Chemical properties of elements properties of elements of the elements depedns on the number of electrons and their arrangement.

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10
Q

According to which law,modern perioidc table is arranged?

A

Modern perioidic law -> Physical and Chemical prop. are perioidic functions of their atomic number.

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11
Q

Perioidic table based on the fundamental property ->

A

Atomic numbers

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12
Q

How does the position of the element corellate?

A

It correlates with its electronic config.

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13
Q

___ horizontal rows are called ____.

____ vertical columns are called ____.

A

7, Periods.

18, Groups.

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14
Q

Each period begins and ends with ___ and ___ respectively.

Each vertical columns with ____ due to their ____.

A

Element having 1 electron; 0 Group -> Completely filled.

similar prop. ; Aame electronic configuration.

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15
Q

Transition from ___ to ___ is seen across a period.

A

Metallic to non-metallic

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16
Q

“Across a period” is always

A

From left to right

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17
Q

What are the normal elemetnts?

A

1, 2, 3 and 13 to 17 (IA to VIIA)

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18
Q

What are transition elements?

A

3 to 12 (IB to VIII)

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19
Q

How many group has transition elements?

A

10 groups

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20
Q

What are the Noble or Inert Gases?

A

18 (zero)

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21
Q

Where are the following placed in the periodic table?

  1. Reactive metals
  2. Transition elements
  3. Non-Metals
A
  1. 1 and 2
  2. 3 to 12 (middle)
  3. Upper right corner
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22
Q

Name the difference/length of periods:

A

2, 8, 8, 18, 18, 32

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23
Q

Gradual change in properties is seen with

A

Increase in atomic number.

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24
Q

Define a period:

A

Seven horizontal rows of the perioidc table

Arranged in inreasing of at. nos

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25
Q

Number of period is equal to

A

The number of shells in the atoms.

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26
Q

Give the range of Lanthanide and Actinide series:

A

58 to 71

90 to 103

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27
Q

What are bridge elements and where are they found?

A

Show similarities -> properties diagnolly with the period with the next group. They are found in perioid 2.

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28
Q

What are typical elemetns and where are they found?

A

They are representatice elements of the respective group and they are found in PERIOD 3

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29
Q

Give the pairs of bridge elements:

A
  1. Li and Mg
  2. Be and AL
  3. B and Si
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30
Q

Lanthanide series is also called ___.

Actinide series is aslo called _____.

A

Rare earth elements

Radio active elements

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31
Q

Boron is a __ .
Silicon is a ___ .
Their positions

A

Metalloid (IIIA)

Metalloid (IVA)

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32
Q

Covalent bonds with Cl is always ___ in room temperature. Except __ whihc is ___

A

Liquid or gas. PCl5. Solid.

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33
Q

Is AlCl3 Ionic or covalent compound?

What is its state?

A

Both. Ionic and Covalent. Solid state.

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34
Q

Al2O3 or Al(OH)3 is ___ compound. But SiO2 is ___.

A

Amphoteric. Weak acid.

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35
Q 
Classify the following:
NaH
MgH2
AlH3
SiH4
PH3
H2S
HCl
A 
Strong base
Weak base
Weaker base
Weaker base
Weaker base
Weak acid
Strong Acid.
(The H needs to be in the front)
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36
Q

Give the chemical formulas for the following compounds:

  1. Metasilisisic Acid
  2. Perchloric acid
  3. Chlorine Heptoxide
  4. Phosphine
  5. Metaphosporic acid
  6. Orthophosphoric acid
A
  1. H2SiO3
  2. HClO4
  3. Cl2O7
  4. PH3
  5. HPO3
  6. H3PO4
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37
Q

Define groups

A

18 vertical columns in the perioidc table.

Signifies the number of valence electrons of an element.

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38
Q

Number of Main Groups

39
Q

Name the location of the following:

  1. Alkali Metals
  2. Alkalie earth metals
  3. Transition elements.
  4. Post transition elements
  5. Halogens
  6. Noble or Inert Gases.
A
  1. 1 or IA
  2. 2 or IIA
  3. 3 to 12 [IB to VIIB and VIII]
  4. 13 to 16 [3A to 6A]
  5. 17 [VIIA]
  6. 18 [0]
40
Q

What are the inner transition metals>O?

A

Lanthanide and Actinide series

41
Q
  1. 1 or IA
  2. 2 or IIA
  3. 3 to 12 [IB to VIIB and VIII]
  4. 13 to 16 [3A to 6A]
  5. 17 [VIIA]
  6. 18 [0]
A
  1. Alkali Metals
  2. Alkalie earth metals
  3. Transition elements.
  4. Post transition elements
  5. Halogens
  6. Noble or Inert Gases.
42
Q

Transition elements:
where do they lie?
What is their similar property?

A

Between the electropositive and least electropositive.

Electron change occurs in the inner orbitals.

43
Q

Lanthanide and Actinide series have ___ elements each.

44
Q

____ remains the same for elements in a ssub-group.

Chemical Properties of elements in a sub-group remains ____ , As it is dependent on

A

Valence Electrons
Simialar (vary gradually)
electronic config.

45
Q

Metallic character ___ and No of electron shell ___. Down a group

A

Increases. Increases by one.

46
Q

Halogen’s state:

A

F, Cl -> Gas
Br -> Liquid
I -> Solid

47
Q

Light soft metals are ___. They can be cut using a ___.

A

1A elements. Knife.

48
Q

Are halogens good conductors of heat and electricity?

49
Q

Halogens are ___ agents.

1A metals are __ agents.

A

Oxidising agent

Reducing agent

50
Q

What does periodicity in properties of elements means?

A
  1. Occurance -> Characterastic prop. of elements
  2. Definite intervals ->
  3. Elements arranged in atomic number (inc. order)
51
Q

The properties that appear in regular interval is ___.

This phenomenon is called ___.

A

Periodic Properties

Periodicity in properties of elements.

52
Q

What are the perioidic properties.

A
  1. Atomic Radius
  2. Ionization potential
  3. Electron affinity
  4. Electronegativity
  5. Metallic or Non-Metallic character
  6. Density
  7. MP or BP
  8. Nature of oxides, hydrides and Oxy-acids
53
Q

What are the reasons for the periodicity?

A
  1. Definite interevals -> Similar valence shells.
  2. => Properties of elements depends on number and arrangement of electrons in various shells including the valence shell
  3. Increase or decrease in a particular prop in the same group or period -> Gradual change in electronic config.
54
Q

Properties of elements depend on the number and arrangement of elements only in valence shell.
True or False.

A

FALSE. Various shells including the valence shells.

55
Q

Unit of atomic radii

56
Q

Atomic radius is

A

Distance between the outermost shell of an atom and the nucleus

57
Q

Atomic radius determines

A

Bond Length

58
Q

Factos which affect atomic radius is

A

Number of shells

Nuclear charge

59
Q

Nuclear charge ->

A

Positivie charge of the nucleus of an atom

Equivalent to the atomic number.

60
Q

In period 2 __ has the largest atomic radii and ___ had the smallest.

61
Q

Neon has a Larger radii, Why?

A

Outershell -> Completely filled => Force of repulsion

Effect of nuclear pull is not seen.

62
Q

Cation is ____ than the actual atom.

Why?

A

Smaller. There is a strong force of attraction by the nucleus. (increase in nuclear charge)

63
Q

Down a grouP -> Increase in ___ dominates over, increase in ___, for atomic radii.

A

number of shells; Nuclear charge;

64
Q

Unit of IP

65
Q

Ionization potential is

A

The amount of energy required to remove a loosely bound electron from the outermost shell of an islated gaseous atom.

66
Q

Energy required to remove the first electron is ___
Energy required to remove the 2nd electron is ___.
___ is greater than ___.

A

First IP; Second IP;

Second IP and First IP;

67
Q

Factors affecting the IP

A

Atomic size -> Higher the size, lower the nuclear attraction.
Nucear charge -> Higher the nuclear charge -> More firly held.

68
Q

___ has the highest IP and __ has the lowest IP.

A

Helium; Caesium;

69
Q

___ is radioactive, as a result Caesium has the lowest IP.

70
Q

Down a group, Increase in ___ dominates over ___ Increase in ___, in IP, EN and EA

A

Atomic Radii, Nuclear charge.

71
Q

Unit of electron affinity and the sign

A

eV; Always -ve or 0;

72
Q

What is electron affinity?

A

Energy released when atom in gas state accepts an electron to form anion.
Tendency of atoms to accept electrons.

73
Q

Factors affecting the EA

A

Atomic size -> Tendency of atoms to take up electron increases with Decrease in atomic size.
Nucear charge -> Tendency of atoms to take up electron increases with increase in Nuclear charge

74
Q

Ionization potential is the tendency of electrons __ electrons, put in energy value.

A

not give out electrons

75
Q

Neon has electron affinity ___.

Why?

A

Zero. Inert gases do not accept electrons and form ions.

76
Q

Electron affinity is Highest for ___ and lowest for ___.

A

Halogens and Alkali metals.

77
Q

Greater the Value of EA -> ____ the value of Electronegativity or oxidising capacity

78
Q

According to the values, which has the highest EA ->

79
Q

Electronegativity:

A

Tendency of an atom to attract electron to itself when combined in a compound
Net result of the tendency of electron to attract the bond forming the electron pair.

80
Q

Electronegativity is ____ for halogens.

81
Q

The amount of energy released on taking up the electron is highest for ____.
The tendency of atom to attract electron to itself is highest in __.
The tendency of the atom to take up electrons is highest in ___.

A

Chlorine.
Fluorine
Chlorine.

82
Q

Which is the most and least electronegative element.

A

Fluorine and Caesium respectively.

83
Q

Noble gases have electronegativity ->

A

Do not attract electrons. So “ - “.

84
Q

Noble gases have electronegativity zero.

True or False.

A

False! They dont have electronegativity.

85
Q

Metal __ electrons. Non-metals __ electrons. Only If it is _____

A

Lose; Gain; Supplied with energy;

86
Q

Reactivity is defined different ways for metals and Non-metals.

87
Q

Reactivity of metals ->

Reactivity of Non-Metals ->

A

Greater the tendency to lose electrons

Greater the tendency to gain electrons.

88
Q

Metals are ____ agents. It has a ___ IP, ___ EA and ___ EN.
Non-Metals are ___ agents. It has a ___ IP, ___ EA and ___ EN.

A

Reducing agents, Oxidising agents.
Low, Low, Low
High, High, High

89
Q

Metals’ atomic radii are ___ than the non-metals of the same period.

90
Q

The periodic properties of the following:

  1. MP
  2. BP
  3. Density
A
  1. Increases across a period and Decreases down a group
  2. Increases across a period and Decreases down a group
  3. Increases across a period and Increases down a group
91
Q

Down a group -> Ph ___. Except for ___.

A

Increases. Hydrides.

92
Q

Across a period -> Ph

A

decreases.

93
Q

We check the ___ ratio to check whether an element is light or heavy.

A

neutron/proton

Chemistry (6 decks)

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