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Questions and Answers
What is the primary reason for the decrease in atomic radius from left to right across a period?
What is the primary reason for the decrease in atomic radius from left to right across a period?
Who is credited with developing the Law of Octaves, which stated that elements exhibited similar properties at intervals of 8?
Who is credited with developing the Law of Octaves, which stated that elements exhibited similar properties at intervals of 8?
Which of the following is a characteristic of metals?
Which of the following is a characteristic of metals?
What is the primary reason for the increase in ionization energy from left to right across a period?
What is the primary reason for the increase in ionization energy from left to right across a period?
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What is the primary function of protons in an atom?
What is the primary function of protons in an atom?
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What is the trend of electronegativity down a group?
What is the trend of electronegativity down a group?
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Which of the following elements is most likely to be a metalloid?
Which of the following elements is most likely to be a metalloid?
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What is the primary reason for the increase in electron affinity from left to right across a period?
What is the primary reason for the increase in electron affinity from left to right across a period?
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Who developed the modern periodic table, which organized elements by atomic weight and chemical properties?
Who developed the modern periodic table, which organized elements by atomic weight and chemical properties?
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What is the characteristic of nonmetals that distinguishes them from metals?
What is the characteristic of nonmetals that distinguishes them from metals?
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Study Notes
Periodic Trends
-
Atomic Radius:
- Decreases from left to right across a period due to increased nuclear charge and decreased shielding.
- Increases down a group due to increased shielding and energy levels.
-
Electronegativity:
- Increases from left to right across a period due to increased nuclear charge and decreased shielding.
- Decreases down a group due to increased shielding and energy levels.
-
Ionization Energy:
- Increases from left to right across a period due to increased nuclear charge and decreased shielding.
- Decreases down a group due to increased shielding and energy levels.
-
Electron Affinity:
- Increases from left to right across a period due to increased nuclear charge and decreased shielding.
- Decreases down a group due to increased shielding and energy levels.
Periodic Table History
-
Early Development:
- John Newlands (1863): Developed the Law of Octaves, which stated that elements exhibited similar properties at intervals of 8.
- Julius Lothar Meyer (1864): Developed an early periodic table, but it was not widely accepted.
-
Mendeleev's Contribution:
- Dmitri Mendeleev (1869): Developed the modern periodic table, which organized elements by atomic weight and chemical properties.
- Predicted the existence of undiscovered elements and left gaps in the table for them.
Element Classification
-
Metals:
- Typically shiny, malleable, and good conductors of electricity.
- Found on the left side and center of the periodic table.
-
Nonmetals:
- Typically dull, brittle, and poor conductors of electricity.
- Found on the right side of the periodic table.
-
Metalloids:
- Exhibits some properties of metals and some properties of nonmetals.
- Found on the border between metals and nonmetals.
Atomic Structure
-
Protons, Neutrons, and Electrons:
- Protons: positively charged, found in the nucleus, and determine the element.
- Neutrons: no charge, found in the nucleus, and contribute to the element's mass.
- Electrons: negatively charged, found in energy levels, and determine the element's chemical properties.
-
Energy Levels and Subshells:
- Energy levels (n): the distance of an electron from the nucleus.
- Subshells (l): the shape of the electron's orbit around the nucleus.
- Orbitals: the specific path of an electron within a subshell.
Periodic Trends
- Atomic radius decreases from left to right across a period due to increased nuclear charge and decreased shielding.
- Atomic radius increases down a group due to increased shielding and energy levels.
- Electronegativity increases from left to right across a period due to increased nuclear charge and decreased shielding.
- Electronegativity decreases down a group due to increased shielding and energy levels.
- Ionization energy increases from left to right across a period due to increased nuclear charge and decreased shielding.
- Ionization energy decreases down a group due to increased shielding and energy levels.
- Electron affinity increases from left to right across a period due to increased nuclear charge and decreased shielding.
- Electron affinity decreases down a group due to increased shielding and energy levels.
Periodic Table History
- John Newlands developed the Law of Octaves in 1863, stating that elements exhibit similar properties at intervals of 8.
- Julius Lothar Meyer developed an early periodic table in 1864, but it was not widely accepted.
- Dmitri Mendeleev developed the modern periodic table in 1869, organizing elements by atomic weight and chemical properties.
- Mendeleev predicted the existence of undiscovered elements and left gaps in the table for them.
Element Classification
- Metals are typically shiny, malleable, and good conductors of electricity, found on the left side and center of the periodic table.
- Nonmetals are typically dull, brittle, and poor conductors of electricity, found on the right side of the periodic table.
- Metalloids exhibit some properties of metals and some properties of nonmetals, found on the border between metals and nonmetals.
Atomic Structure
- Protons are positively charged, found in the nucleus, and determine the element.
- Neutrons have no charge, are found in the nucleus, and contribute to the element's mass.
- Electrons are negatively charged, found in energy levels, and determine the element's chemical properties.
- Energy levels (n) refer to the distance of an electron from the nucleus.
- Subshells (l) refer to the shape of the electron's orbit around the nucleus.
- Orbitals refer to the specific path of an electron within a subshell.
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