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Questions and Answers
What is the relationship between relative atomic mass, abundance percentage, and atomic mass?
What is the relationship between relative atomic mass, abundance percentage, and atomic mass?
Which group in the periodic table is known for being highly reactive and easily losing their outer electron?
Which group in the periodic table is known for being highly reactive and easily losing their outer electron?
What property increases as you move down Group 1 – Alkali Metals in the periodic table?
What property increases as you move down Group 1 – Alkali Metals in the periodic table?
Which group in the periodic table has a valence of 2 and is shiny?
Which group in the periodic table has a valence of 2 and is shiny?
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Why are isotopes considered to be the same chemically but not physically?
Why are isotopes considered to be the same chemically but not physically?
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Which group in the periodic table has a valence of 7 and can be solid, liquid, or gas?
Which group in the periodic table has a valence of 7 and can be solid, liquid, or gas?
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Why do atomic radii increase down a group?
Why do atomic radii increase down a group?
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What causes atomic radii to decrease from left to right across a period?
What causes atomic radii to decrease from left to right across a period?
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What is the main characteristic of noble gases in terms of reactivity?
What is the main characteristic of noble gases in terms of reactivity?
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What feature distinguishes lanthanides and actinides from other elements?
What feature distinguishes lanthanides and actinides from other elements?
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What is the effect of the release of radiation by radioactive elements?
What is the effect of the release of radiation by radioactive elements?
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In metallic bonding, what property arises from the delocalized electrons?
In metallic bonding, what property arises from the delocalized electrons?
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Study Notes
Relative Atomic Mass
- Calculated by: (abundance percentage x atomic mass) + (abundance percentage x atomic mass) / 100
- Used to determine the average mass of an element
Characteristics of Atoms
- Chemical nature depends on the number of electrons
- Isotopes have the same chemical properties but different physical properties due to varying numbers of neutrons
Periodic Table Group Properties
Group 1 - Alkali Metals
- Valence: 1
- Highly reactive, easily lose their outer electron to obtain a complete outer shell
- Not readily found in nature
- Reactivity increases as you move down the group (ionization energy decreases)
- Good conductors of heat and electricity
- Soft and malleable
Group 2 - Alkaline Earth Metals
- Valence: 2
- Highly reactive, easily lose their outer electron to obtain a complete outer shell
- Not readily found in nature
- Reactivity increases as you move down the group (ionization energy decreases)
- Good conductors of heat and electricity
- Shiny
Group 7 - Halogens
- Valence: 7
- May be solid, liquid, or gas
- Highly reactive, strong electronegativity (tends to 'steal' electrons from other elements)
Group 8 - Noble Gases
- Maximum number of electrons in outer shell
- Extremely high ionization energy
- Unreactive
Transitional Metals
- Can have multiple valencies (e.g. Fe: Fe2+, 3+)
- Good conductors of heat and electricity
- Malleable and ductile
Lanthanides and Actinides
- Have 2 electrons in outer shell
- Good electrical conductors
- Silver: tarnishes easily
Radioactive Elements
- Have more than 82 protons
- Unstable nuclei due to proton-to-neutron ratio
- Release radiation and may have short or long half-lives
Atomic Radius
- Increases down a group due to additional energy levels and electrons
- Decreases from left to right across a period due to electrostatic attractions
Ionic Charge and Radius
- Atoms tend to lose or gain electrons to achieve complete s and p sublevels
Bonding
Metallic Bonding
- Involves the electrostatic attraction between metal ions that have released electrons
- Valence electrons are loosely held as metal (low ionization energy)
- Forms positively charged cations
- Delocalized electrons are free to move randomly
- Overall neutral charge (number of cations = number of delocalized electrons)
- Non-directional
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Description
Learn how to calculate the relative atomic mass of an element using the formula provided in the image. Understand how the abundance percentage and atomic mass of isotopes contribute to determining the relative atomic mass.
