Periodic Table & Chemistry Flashcards

Periodic Table & Chemistry Flashcards
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Define the term: metalloid
Elements that share characteristics with metals and non-metals. They are on the 'steps' of the stairstep line that divides metals and nonmetals on the periodic table.
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Difficulty of ionizing Group 2 elements
Ionizing Group 2 elements is relatively easy, compared to others in the same row.
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Describe the change in atomic radius/size within a period (row) of the periodic table.
Atoms with more protons (toward the right side of the table) are smaller, because the greater number of protons can pull harder on the electrons.
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Define the term: Main group element
Elements with electron configurations in which the last electron is in the s block or the p block
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Define the term: Transition metals
Elements in the d-block of the periodic table. They have partly filled d orbitals.
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The reason why electronegativity changes as you move left-to-right along the periodic table (within the same row)
With more protons in the nucleus, the nucleus can exert greater pull on the electrons.
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The reason why electronegativity changes as you go down a column of the periodic table
In small atoms, the electrons are closer to the nucleus, which can tug on the electrons harder.
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The change in ionization energy as you go top-to-bottom down the periodic table, within the same group (column)
Ionization energy decreases.
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The change in ionization energy as you go left-to-right along the periodic table, within the same period (row)
Ionization energy increases.
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Flashcard Content Overview

With these flashcards, you will test your knowledge of two elemental characteristics: ionization energy and electronegativity. The cards will help you confirm that you understand how these characteristics change as you go across and down the periodic table. You'll learn the difference between first and second ionization energy.

You can review the surprising ways that atomic radius and ionic radius differ between elements of the same period.

Other flashcards in the set will help you remember the differences between the types of element on the periodic table, including main group elements, transition metals, and metalloids.

Front
Back
The change in ionization energy as you go left-to-right along the periodic table, within the same period (row)
Ionization energy increases.
The change in ionization energy as you go top-to-bottom down the periodic table, within the same group (column)
Ionization energy decreases.
The reason why electronegativity changes as you go down a column of the periodic table
In small atoms, the electrons are closer to the nucleus, which can tug on the electrons harder.
The reason why electronegativity changes as you move left-to-right along the periodic table (within the same row)
With more protons in the nucleus, the nucleus can exert greater pull on the electrons.
Define the term: Transition metals
Elements in the d-block of the periodic table. They have partly filled d orbitals.
Define the term: Main group element
Elements with electron configurations in which the last electron is in the s block or the p block
Describe the change in atomic radius/size within a period (row) of the periodic table.
Atoms with more protons (toward the right side of the table) are smaller, because the greater number of protons can pull harder on the electrons.
Difficulty of ionizing Group 2 elements
Ionizing Group 2 elements is relatively easy, compared to others in the same row.
Define the term: metalloid
Elements that share characteristics with metals and non-metals. They are on the 'steps' of the stairstep line that divides metals and nonmetals on the periodic table.
Number of valence electrons in elements from Group 14 of the periodic table
Four valence electrons
How an atom's radius changes when it becomes an ion
Positive ions have lost electrons, so their radii get smaller. Negative ions have gained electrons, so their radii get bigger.
How electronegativity changes left-to-right across the periodic table
Electronegativity increases
How electronegativity changes as you go down the periodic table (within the same column).
Electronegativity decreases.
This orbital holds the last valence electron of an alkali earth metal atom
An s orbital
How atomic radius changes within a group (column) as you go down the periodic table.
Atomic radius increases.
First ionization energy
The energy required to remove a single electron from an atom or element
Second ionization energy
The energy required to remove a second electron for an atom or element
Elements that typically have the lowest second ionization energies
Alkaline earth metals

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