Podcast
Questions and Answers
Why do atoms lose, gain, or share electrons?
Why do atoms lose, gain, or share electrons?
- To achieve a stable, full outer shell of electrons, like noble gases (correct)
- To decrease their atomic radius
- To increase their reactivity with other elements
- To become less stable and more unpredictable
Noble gases readily lose, gain, or share electrons to form chemical bonds.
Noble gases readily lose, gain, or share electrons to form chemical bonds.
False (B)
What is the 'octet rule'?
What is the 'octet rule'?
Atoms aim to have eight electrons in their outer shell to achieve stability.
The atomic radius of an atom is the distance from its _______ to the outermost _______.
The atomic radius of an atom is the distance from its _______ to the outermost _______.
Match the group with the description:
Match the group with the description:
What happens to the atomic radius as you move down a group in the periodic table?
What happens to the atomic radius as you move down a group in the periodic table?
What is the relationship between atomic radius and reactivity in Group 1 alkali metals?
What is the relationship between atomic radius and reactivity in Group 1 alkali metals?
The reactivity of elements in Groups 1 and 2 decreases as you move down the group.
The reactivity of elements in Groups 1 and 2 decreases as you move down the group.
Why does the reactivity of Group 1 metals increase as you move down the group?
Why does the reactivity of Group 1 metals increase as you move down the group?
Alkali metals have _______ valence electron in their outer shell, making them highly _______. They easily _______ this electron to achieve a stable, full outer shell.
Alkali metals have _______ valence electron in their outer shell, making them highly _______. They easily _______ this electron to achieve a stable, full outer shell.
Flashcards
Octet Rule
Octet Rule
Atoms gain, lose, or share electrons to achieve a full outer shell, resembling stable noble gases.
Atomic Radius
Atomic Radius
Distance from the nucleus to the outermost electrons, indicating atom size; increases down a group, decreases across a period.
Alkali Metals (Group 1)
Alkali Metals (Group 1)
Elements with one valence electron that readily lose it, forming positive ions and reacting with other elements.
Group 1 & 2 Reactivity Trend
Group 1 & 2 Reactivity Trend
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Atomic Radius and Reactivity
Atomic Radius and Reactivity
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Study Notes
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Noble gases possess complete outer shells and do not readily lose, gain, or share electrons.
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Atoms seek stability by achieving a full outer shell of electrons, similar to noble gases.
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The octet rule describes the tendency of atoms to gain eight electrons in their outer shell.
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Atomic radius measures the distance from the nucleus to the outermost electrons, indicating atom size.
Periodic Table Trends
- Atomic radius increases down a group in the periodic table.
- Atomic radius decreases across a period from left to right in the periodic table.
Group 1 Alkali Metals
- Group 1 alkali metals have one valence electron in their outer shell, making them highly reactive.
- They easily lose this single electron to achieve a stable, full outer shell.
- They readily form positive ions and quickly react with elements like halogens to form compounds.
Reactivity Trends
- As you move down Group 1 and Group 2, the reactivity of elements increases.
- Outer electrons are further from the nucleus, making them easier to lose due to weaker attraction.
- Additional electron shells reduce the pull from the nucleus on outer electrons.
Reactivity and Atomic Radius
- As atomic radius increases, outer electrons are further from the nucleus.
- Greater distance weakens the attraction between the nucleus and outer electrons, making it easier to lose electrons.
- In Group 1, metals become more reactive moving down the group.
- In Group 2, metals also become more reactive moving down the group due to the same reason.
Analyzing Graphs and Charts
- Determine the independent and dependent variables.
- Identify the type of graph or chart used and the reason for its selection.
- Determine which value or data point is the highest and how you know.
- Calculate the total amount or sum of all values.
Comparative Analysis
- Describe the change from one point or period to another.
- Note any unusual or unexpected observations.
Trend Identification
- Describe the general trend observed in the data.
- Verify if all data points follow the trend and provide supporting evidence.
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