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Semeter 2 EXAMS - Science (2024) > 5.2 Arranging the elements 5.3 Family grouping > Flashcards

5.2 Arranging the elements 5.3 Family grouping Flashcards

Slide 3.1 b

1
Q

Periods in the Periodic Table

A

The horizontal rows in the periodic table are called periods. They are numbered 1 to 7.

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2
Q

Number of Groups

A

There are 18 groups (vertical columns) in the periodic table, numbered from 1 to 18 or using Roman numerals I to VIII.

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3
Q

Periodic Table Organization

A

Elements are arranged in the periodic table based on the arrangement of periods (horizontal rows) and groups (vertical columns).

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4
Q

Example - Oxygen (O)

A

Oxygen (O) is located in period 2, group 16 of the periodic table.

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4
Q

Elements in the Same Group

A

Elements in the same group of the periodic table have similar physical and chemical properties. For example, Group 2 contains metals that react in a similar way and form very similar compounds.

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5
Q

Group Similarities

A

Elements in the same group, while not identical, share similar characteristics and properties due to their arrangement in the periodic table.

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6
Q

Special Blocks

A

The transition elements, the lanthanides, and the actinides are placed in special blocks within the periodic table.

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7
Q

Transition Elements

A

The transition elements are placed in the central block of the periodic table.

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8
Q

Lanthanides

A

The lanthanides are placed in a separate block below the main periodic table.

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9
Q

Actinides

A

The actinides are placed in a separate block below the lanthanides, also outside the main periodic table.

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10
Q

Group 1 - Alkali metals

A

Highly reactive
Soft, low-melting solids
React violently with water

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11
Q

Group 2 - Alkaline earth metals

A

Moderately reactive
Low-melting solids
React with water to form basic solutions

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12
Q

Group 13 - Boron group

A

Metalloids and nonmetals
Semiconductors
Includes boron, aluminum, gallium

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13
Q

Group 18 - Noble gases

A

-Unreactive, stable elements
Colorless, odorless gases
Includes helium, neon, argon

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14
Q

Alkali Metal Properties

A
  • Form ions with a charge of +1
  • Have typical metallic properties
  • Display similar extreme chemical behavior
  • Too reactive to be found naturally in pure forms
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15
Q

Reactivity of Alkali Metals

A
  • Highly reactive group of elements
  • Cannot be found naturally in pure form due to reactivity
  • Easily form positive ions (+1 charge)
  • Exhibit characteristic metallic properties
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16
Q

Alkali Metal Examples

A

Lithium (Li)
Sodium (Na)
Potassium (K)
Rubidium (Rb)
Cesium (Cs)
Francium (Fr)

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17
Q

Alkali Metal Reactivity

A
  • Extremely reactive with water, forming basic solutions
  • React violently with many other substances
  • Require special storage and handling to prevent reactions
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18
Q

Density of Alkali Metals

A
  • Lithium, Sodium, and Potassium are less dense than water
  • This allows them to float on water
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18
Q

Reactivity of Alkali Metals

A
  • Alkali metals are soft and reactive
  • React with chlorine gas to form white salt compounds
  • Reactions shown with chlorine, bromine, and fluorine
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19
Q

Sodium Reactions

A

Sodium + Chlorine → Sodium Chloride (NaCl)
2Na + Cl2 → 2NaCl

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20
Q

Potassium Reactions

A

Potassium + Bromine → Potassium Bromide (KBr)
2K + Br2 → 2KBr

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21
Q

Lithium Reactions

A

Lithium + Fluorine → Lithium Fluoride (LiF)
2Li + F2 → 2LiF

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22
Q

Alkali Metal Reactivity with Water

A
  • Alkali metals react violently with water
  • Produce an alkaline or basic solution
  • Generate hydrogen gas as a byproduct
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23
Sodium Reaction with Water
- Sodium + Water → Sodium Hydroxide + Hydrogen Gas - 2Na + 2H2O → 2NaOH + H2
24
Lithium Reaction with Water
- Lithium + Water → Lithium Hydroxide + Hydrogen Gas - 2Li + 2H2O → 2LiOH + H2
25
Potassium Reaction with Water
- Potassium + Water → Potassium Hydroxide + Hydrogen Gas - 2K + 2H2O → 2KOH + H2
26
Electron Structure of Alkali Metals
- All alkali metals have 1 electron in their outer shell - They can easily obtain a full outer shell by losing 1 electron - They all lose their outer shell electron in reactions to form positive ions with a +1 charge - They have similar physical and chemical properties
27
Lithium Electron Configuration
Lithium has 2 electrons in the inner shell and 1 electron in the outer shell (2,1)
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Sodium Electron Configuration
Sodium has 2 electrons in the inner shell and 8 electrons in the outer shell (2,8,1)
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Potassium Electron Configuration
Potassium has 2 electrons in the inner shell, 8 in the middle shell, and 1 in the outer shell (2,8,1)
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Atom Size and Electron Shells
- The size of the element's atoms increases down the group - The number of full electron shells also increases down the group - This means the valence electron is further from the nucleus and more shielded
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Valence Electron Shielding
- The valence electron is further away from the nucleus and shielded by more inner electron shells - This makes the valence electron less tightly bound to the nucleus
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Ease of Electron Loss
- The further the valence electron is from the nucleus, the easier it can be lost in reactions - This increases the reactivity of the alkali metals down the group
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Increased Reactivity
- The increased shielding and weaker attraction to the nucleus means reactivity increases with the size of the atom - Reactivity goes up as you move down the group of alkali metals
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Atom Size and Group Position
- Atoms get larger as you move down a group in the periodic table - This increase in atom size causes metals to become less stable and more reactive
34
Increased Reactivity Down the Group
- The larger atom size and more shielded valence electrons make the metals down the group more likely to react with other substances - This is why reactivity increases as you go down the group
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Sodium vs Lithium Reactivity
- Sodium reacts much more violently than lithium in both air and water - The alkali metals are stored in paraffin oil to keep them moisture-free due to their instability
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Alkaline Earth Metals
- The alkaline earth metals are all metals that act in a slightly less reactive way compared to the alkali metals - They are found in Group 2 of the periodic table
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Reactivity of Alkaline Earths
When the alkaline earth metals react, they lose two electrons from each atom This allows them to form ions with a charge of +2
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Electron Configuration
- The alkaline earth metals have 2 electrons in their outer shell - They lose these 2 electrons in reactions to form positive +2 ions
39
Group 2 Examples
Examples of alkaline earth metals include: - Beryllium (Be) - Magnesium (Mg) - Calcium (Ca) - Strontium (Sr) - Barium (Ba) - Radium (Ra)
40
Group 14 Elements
- The Group 14 elements display a wide range of properties. - They include carbon, silicon, germanium, tin, and lead.
41
Carbon Allotropes
- Carbon has different forms or allotropes. - The most common allotropes are charcoal, diamond, graphite, and buckyballs.
42
Organic Substances
- Substances with molecules containing carbon atoms are known as organic substances. - Organic molecules make up all living things.
43
Group 14 Elements in Technology
- Diamond is a form of carbon used in electronic circuit chips. - Silicon is used in electronic circuit chips. - Lead is used in car batteries. - Carbon, silicon, and lead are all Group 14 elements.
44
Atoms of Halogens
- Form ions with a charge of -1 - Are not found in pure form, but in various salts (NaCl) - Get bigger and become less reactive as you move down the group
45
Halogen Molecules
- Form molecules that are made up of two atoms (Cl2, Br2) - Produce coloured and poisonous vapours
46
Properties of Halogens
- The halogens have similarities, but their different sizes result in some differences in their properties.
47
Physical States of Halogens
- Halogens represent all three familiar states of matter: 1. Chlorine is a gas 2. Bromine is a liquid 3. Iodine is a solid
48
Halogen Reactivity
The halogens become less reactive as you move down the group (from chlorine to iodine).
49
Halogen Properties
- Halogens form ions with a charge of -1. - Halogens are not found in pure form, but in various salts (e.g. NaCl). - Halogen molecules are made up of two atoms (Cl2, Br2). - Halogens produce colored and poisonous vapors.
50
Noble Gases
- The noble gases are also known as the inert gases. - They are colourless and occur naturally in the atmosphere. - They are very stable and react only under rare or extreme circumstances.
51
Properties of Noble Gases
- Colourless - Occur naturally in the atmosphere - Very stable - React only under rare or extreme circumstances
52
Noble Gases in the Periodic Table
- The noble gases are located in Group 18 of the periodic table. - They include helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).
53
Density of Noble Gases
- Helium has a lower density than air, which is why helium balloons float up into the air. - As you move down the group, the other noble gases get progressively denser and thus the balloons are heavier.
53
Noble Gas Densities
The atoms of the noble gases get bigger and heavier as you move down the group, making them denser and less likely to float in air.
54
Helium's Low Density
Helium has a lower density than air, which is why helium balloons float up into the air.
55
What are the transition elements?
The transition elements are all metals.
56
What are some examples of useful, colorful, and valuable transition metals?
Iron, copper, zinc, gold, and silver are some examples of useful, colorful, and valuable transition metals.
57
What are some common properties of transition metals?
Transition metals tend to be relatively hard and have high melting points.
58
How can transition metal compounds appear?
Transition metal compounds can have very colorful appearances, as shown in the solutions of nickel, chromium, cobalt, and vanadium.
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Semeter 2 EXAMS - Science (2024) (7 decks)

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