1 Periodic Table Flashcards
1
Q
What was the need that arose?
A
To group the elements into families whose elements showed maximum rsemblance.
2
Q
Early chemists: 1. Basis of arranging 2 Method of arranging 3. Reason for discarding 4. Year
A
- On the basis of valency, metallic or non-metallic character.
- -
- Showed Variable Valency and dual character (metalloids).
- -
3
Q
Dobreiner: 1. Basis of arranging 2 Method of arranging 3. Reason for discarding 4. Year
A
- Atomic weights -> Increasing order
- Triads; At. weight of the middle element is average of the other two.
- It didnt hold true for all the elements.
- 1815
4
Q
Newland: 1. Basis of arranging 2 Method of arranging 3. Reason for discarding 4. Year
A
- Atomic weights -> Increasing order
- Series of eight; Property of every 8th element is the property of the 1st element.
- Didnt leave space for undiscovered elements.
- 1864
5
Q
Medeleef: 1. Basis of arranging 2 Method of arranging 3. Reason for discarding 4. Year
A
- Atomic weights -> Increasign order.
- In a table -> Mendeleef’s periodic table. Properties are periodic funcions of at. weight.
- Mehtod couldnt justify -> Certain elements, rare earth and isotopes.
- 1869
6
Q
Mosley: 1. Basis of arranging 2 Method of arranging 3. Reason for Adopting 4. Year
A
- Increased order of atomic numbers.
- In a table -> Modern periodic table. Properties are perioidc functions of atomic number.
- Method removes most of the defects of mendeleef.
- 1912
7
Q
Which group in older notation has 3 groups?
A
VIII -> 8, 9 and 10
8
Q
In older notation, 18th group is called?
A
0 group.
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.
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.
11
Q
Perioidic table based on the fundamental property ->
A
Atomic numbers
12
Q
How does the position of the element corellate?
A
It correlates with its electronic config.
13
Q
___ horizontal rows are called ____.
____ vertical columns are called ____.
A
7, Periods.
18, Groups.
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.
15
Q
Transition from ___ to ___ is seen across a period.
A
Metallic to non-metallic
16
Q
“Across a period” is always
A
From left to right
17
Q
What are the normal elemetnts?
A
1, 2, 3 and 13 to 17 (IA to VIIA)
18
Q
What are transition elements?
A
3 to 12 (IB to VIII)
19
Q
How many group has transition elements?
A
10 groups
20
Q
What are the Noble or Inert Gases?
A
18 (zero)
21
Q
Where are the following placed in the periodic table?
- Reactive metals
- Transition elements
- Non-Metals
A
- 1 and 2
- 3 to 12 (middle)
- Upper right corner
22
Q
Name the difference/length of periods:
A
2, 8, 8, 18, 18, 32
23
Q
Gradual change in properties is seen with
A
Increase in atomic number.
24
Q
Define a period:
A
Seven horizontal rows of the perioidc table
Arranged in inreasing of at. nos
25
Number of period is equal to
The number of shells in the atoms.
26
Give the range of Lanthanide and Actinide series:
58 to 71
| 90 to 103
27
What are bridge elements and where are they found?
Show similarities -> properties diagnolly with the period with the next group. They are found in perioid 2.
28
What are typical elemetns and where are they found?
They are representatice elements of the respective group and they are found in PERIOD 3
29
Give the pairs of bridge elements:
1. Li and Mg
2. Be and AL
3. B and Si
30
Lanthanide series is also called ___.
| Actinide series is aslo called _____.
Rare earth elements
| Radio active elements
31
Boron is a __ .
Silicon is a ___ .
Their positions
Metalloid (IIIA)
| Metalloid (IVA)
32
Covalent bonds with Cl is always ___ in room temperature. Except __ whihc is ___
Liquid or gas. PCl5. Solid.
33
Is AlCl3 Ionic or covalent compound?
| What is its state?
Both. Ionic and Covalent. Solid state.
34
Al2O3 or Al(OH)3 is ___ compound. But SiO2 is ___.
Amphoteric. Weak acid.
35
```
Classify the following:
NaH
MgH2
AlH3
SiH4
PH3
H2S
HCl
```
```
Strong base
Weak base
Weaker base
Weaker base
Weaker base
Weak acid
Strong Acid.
(The H needs to be in the front)
```
36
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
1. H2SiO3
2. HClO4
3. Cl2O7
4. PH3
5. HPO3
6. H3PO4
37
Define groups
18 vertical columns in the perioidc table.
| Signifies the number of valence electrons of an element.
38
Number of **Main** Groups
8
39
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.
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
What are the inner transition metals>O?
Lanthanide and Actinide series
41
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]
1. Alkali Metals
2. Alkalie earth metals
3. Transition elements.
4. Post transition elements
5. Halogens
6. Noble or Inert Gases.
42
Transition elements:
where do they lie?
What is their similar property?
Between the electropositive and least electropositive.
| Electron change occurs in the inner **orbitals**.
43
Lanthanide and Actinide series have ___ elements each.
14
44
____ remains the same for elements in a ssub-group.
| Chemical Properties of elements in a sub-group remains ____ , As it is dependent on
Valence Electrons
Simialar (vary gradually)
electronic config.
45
Metallic character ___ and No of electron shell ___. Down a group
Increases. Increases by one.
46
Halogen's state:
F, Cl -> Gas
Br -> Liquid
I -> Solid
47
Light soft metals are ___. They can be cut using a ___.
1A elements. Knife.
48
Are halogens good conductors of heat and electricity?
No.
49
Halogens are ___ agents.
| 1A metals are __ agents.
Oxidising agent
| Reducing agent
50
What does periodicity in properties of elements means?
1. Occurance -> Characterastic prop. of elements
2. Definite intervals ->
3. Elements arranged in atomic number (inc. order)
51
The properties that appear in regular interval is ___.
| This phenomenon is called ___.
Periodic Properties
| Periodicity in properties of elements.
52
What are the perioidic properties.
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
What are the reasons for the periodicity?
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
Properties of elements depend on the number and arrangement of elements only in valence shell.
True or False.
FALSE. Various shells including the valence shells.
55
Unit of atomic radii
Angstrom
56
Atomic radius is
Distance between the outermost shell of an atom and the nucleus
57
Atomic radius determines
Bond Length
58
Factos which affect atomic radius is
Number of shells
| Nuclear charge
59
Nuclear charge ->
Positivie charge of the nucleus of an atom
| Equivalent to the atomic number.
60
In period 2 __ has the largest atomic radii and ___ had the smallest.
Li; F;
61
Neon has a Larger radii, Why?
Outershell -> Completely filled => Force of repulsion
| Effect of nuclear pull is not seen.
62
Cation is ____ than the actual atom.
| Why?
Smaller. There is a strong force of attraction by the nucleus. (increase in nuclear charge)
63
Down a grouP -> Increase in ___ dominates over, increase in ___, for atomic radii.
number of shells; Nuclear charge;
64
Unit of IP
eV
65
Ionization potential is
The amount of energy required to remove a loosely bound electron from the outermost shell of an islated gaseous atom.
66
Energy required to remove the first electron is ___
Energy required to remove the 2nd electron is ___.
___ is greater than ___.
First IP; Second IP;
| Second IP and First IP;
67
Factors affecting the IP
Atomic size -> Higher the size, lower the nuclear attraction.
Nucear charge -> Higher the nuclear charge -> More firly held.
68
___ has the highest IP and __ has the lowest IP.
Helium; Caesium;
69
___ is radioactive, as a result Caesium has the lowest IP.
Francium.
70
Down a group, Increase in ___ dominates over ___ Increase in ___, in IP, EN and EA
Atomic Radii, Nuclear charge.
71
Unit of electron affinity and the sign
eV; Always -ve or 0;
72
What is electron affinity?
Energy released when atom in gas state accepts an electron to form anion.
Tendency of atoms to accept electrons.
73
Factors affecting the EA
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
Ionization potential is the tendency of electrons __ electrons, put in energy value.
not give out electrons
75
Neon has electron affinity ___.
| Why?
Zero. Inert gases do not accept electrons and form ions.
76
Electron affinity is Highest for ___ and lowest for ___.
Halogens and Alkali metals.
77
Greater the Value of EA -> ____ the value of Electronegativity or oxidising capacity
Greater
78
According to the values, which has the highest EA ->
Chlorine.
79
Electronegativity:
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
Electronegativity is ____ for halogens.
Highest
81
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 ___.
Chlorine.
Fluorine
Chlorine.
82
Which is the most and least electronegative element.
Fluorine and Caesium respectively.
83
Noble gases have electronegativity ->
Do not attract electrons. So " - ".
84
Noble gases have electronegativity zero.
| True or False.
False! They dont have electronegativity.
85
Metal __ electrons. Non-metals __ electrons. Only If it is _____
Lose; Gain; Supplied with energy;
86
Reactivity is defined different ways for metals and Non-metals.
True.
87
Reactivity of metals ->
| Reactivity of Non-Metals ->
Greater the tendency to lose electrons
| Greater the tendency to gain electrons.
88
Metals are ____ agents. It has a ___ IP, ___ EA and ___ EN.
Non-Metals are ___ agents. It has a ___ IP, ___ EA and ___ EN.
Reducing agents, Oxidising agents.
Low, Low, Low
High, High, High
89
Metals' atomic radii are ___ than the non-metals of the same period.
LARGER
90
The periodic properties of the following:
1. MP
2. BP
3. Density
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
Down a group -> Ph ___. Except for ___.
Increases. Hydrides.
92
Across a period -> Ph
decreases.
93
We check the ___ ratio to check whether an element is light or heavy.
neutron/proton
