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Chemistry Grade 10 > Periodic Table & Periodic Trends > Flashcards

Periodic Table & Periodic Trends Flashcards

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1
Q

Modern Periodic Law

A

“Physical & Chemical properties of elements are periodic functions of their atomic number.”

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2
Q

Moseley Contribution to the Periodic Table

A

He arranged elements in the order of increasing atomic number as the properties of elements depend on their electronic configuration.

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3
Q

Number of Periods

A

7

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4
Q

Number of Groups

A

18

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5
Q

Define: Periodicity

A

Occurrence of characteristic properties of elements at definite intervals in the modern periodic table when elements are arranged in increasing order of their atomic numbers.

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6
Q

Normal Elements Group Number

A

1 & 2, 13 to 17

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7
Q

Transition Elements Group Number

A

3 to 12

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8
Q

Noble or Inert Gases Group Number

A

18

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9
Q

Reactive Elements Group Number

A

1 & 2

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10
Q

Number of Elements in each period

A

2, 8, 8, 18, 18, 32, 26

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11
Q

Bridge Elements

A

ELements in Period 2 show similar properties to the elements diagonal to them in Period 3.

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12
Q

Other name for electropositive nature:

A

Metallic Nature

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13
Q

Other name for electronegative nature:

A

Non-Metallic Nature

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14
Q

Define: Electropositive/ Metallic Nature

A

Property of an element to lose electrons.

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15
Q

Define: Electronegative/ Non-Metallic Nature

A

Property of an element to gain electrons.

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16
Q

Define: Electron Affinity

A

It is the amount of energy released when an atom in the gaseous state accepts an electron to form an anion.

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17
Q

Define: Atomic Radius

A

It is the distance between the centre of the nucleus and the outer most shell of the atom.

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18
Q

Define: Ionisation Potential

A

It is the amount of energy required to to remove an electron from the outer most shell of an isolated gaseous atom.

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19
Q

Define: Electronegativity

A

It is the tendency of an atom to attract electrons to itself when combined in a compound.

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20
Q

Metallic nature __________ across a period from left to right.

A

decreases

21
Q

Non-metallic nature __________ across a period from left to right.

A

increases

22
Q

Metallic nature __________ down a group.

A

increases

23
Q

Non-metallic nature __________ down a group.

A

decreases

24
Q

Element with highest metallic nature :

A

Caesium(natural), Francium(man-made)

25
Q

Element with highest non-metallic nature :

A

Fluorine

26
Q

Atomic size __________ across a period from left to right because ________.

A

decreases , nuclear charge increases

27
Q

Atomic size __________ down a group because ________.

A

increases, number of shells increases

28
Q

Largest Atomic Radius:

A

Francium

29
Q

Smallest Atomic Radius:

A

Helium

30
Q

Ionisation Potential __________ across a period from left to right because ________.

A

increases, atomic size decreases

31
Q

Ionisation Potential __________ down a group because ________.

A

decreases, atomic size increases

32
Q

Highest IP:

A

Helium

33
Q

Lowest IP:

A

Caesium

34
Q

Electron Affinity __________ across a period from left to right because ________.

A

increases, atomic radius decreases

35
Q

Electron Affinity __________ down a group because ________.

A

decreases, atomic radius increases

36
Q

Highest EA:

A

Chlorine

37
Q

Lowest EA:

A

Argon

38
Q

Electronegativity __________ across a period from left to right because ________.

A

increases, atomic radius decreases

39
Q

Electronegativity __________ down a group because ________.

A

decreases, atomic radius increases

40
Q

Highest Electronegativity:

A

Fluorine

41
Q

Lowest Electronegativity:

A

Caesium

42
Q

Na2O Bonding & Character:

A

Electrovalent & Strongly Basic

43
Q

MgO Bonding & Character:

A

Electrovalent & Basic

44
Q

Al2O3 Bonding & Character:

A

Electrovalent & Amphoteric

45
Q

SiO2 Bonding & Character:

A

Covalent & Weakly Acidic

46
Q

P2O5 Bonding & Character:

A

Covalent & Acidic

47
Q

SO2, SO3 Bonding & Character:

A

Covalent & Acidic

48
Q

Cl2O7 Bonding & Character:

A

Covalent & Strongly Acidic

Chemistry Grade 10 (3 decks)

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