Trends in the Periodic Table Flashcards

1
Q

What are trends?

A

Specific patterns found in the periodic table that illustrate different aspects of an element.

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2
Q

Why do these trends exist?

A
  1. Similar atomic structure of elements in their respective groups or periods, due to their arrangement in the periodic table.
  2. Because of the periodic nature of elements.
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3
Q

Why are trends important?

A
  1. Because they help predict the chemical and physical properties of the element.
  2. Trends are based on the periodic law.
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4
Q

What is atomic size?

A

The distance between the nucleus and the outermost electron.

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5
Q

What does the atomic size depend on?

A
  1. No. of energy levels
  2. Proton pulling power
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6
Q

Why does atomic size increase down a group?

A

Because an extra energy level is added, and this decreases over all attraction.

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7
Q

True or False: Atomic size increases left to right, across a period.

A

False.

Because a proton is added, e- is added in the same energy shell

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8
Q

Why is the size of cation less than neutral atom?

A

Because cation has more protons than electrons so effective nuclear charge increases, pulling the electrons closer.

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9
Q

Why is the size of anion greater than neutral atom?

A

Because anion has more electrons than protons, so effective nuclear charge and attraction decrease, increasing the size.

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10
Q

Why does the size of anions decrease across the period?

A

Although no. of electrons exceeds no. of protons, the electrons are added in the same shell, hence, increasing attraction.

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11
Q

What is ionization energy?

A

Ionization energy is the lowest possible energy value required to remove one electron from the outer shell of an atom.

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12
Q

How do Group 1 elements easily form ions?

A

Because they have low values of ionization energy.

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13
Q

Why do Group 18 elements have high values of ionization energy?

A

Because they have a complete octet, which accounts for their high stability and non-reactivity.

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14
Q

What is electronegativity?

A

Ability to attract electrons in a chemical bond

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15
Q

What is electronegativity measured in?

A

In Pauling scale

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16
Q

Why do noble gases do not have any electronegativity values?

A

Because they form rare compounds.

17
Q

What is electron affinity?

A

It is the energy change when an electron is added to an isolated atom.

18
Q

What does high value of electron affinity indicate?

A

Large amount of energy is released when an electron is added, hence, more stability of a negative ion.

19
Q

What are the conditions for the reactivity of metals?

A
  1. Low ionization energy
  2. Low electronegativity
20
Q

What are the conditions for the reactivity of non-metals?

A
  1. High electron affinity
  2. High electronegativity
21
Q

Which is the most electronegative element?

A

Fluorine:
1. Reacts explosively
2. Is not found free in nature
3. It is highly dangerous

22
Q

What are oxidation states?

A

Total number of electrons an atom gains or loses in order to form a chemical bond.