Podcast
Questions and Answers
Which of the following best describes the trend of atomic radius as you move from left to right across a period on the periodic table?
Which of the following best describes the trend of atomic radius as you move from left to right across a period on the periodic table?
- Generally increases due to increasing nuclear charge.
- Varies unpredictably based on electron configuration.
- Generally decreases due to increasing nuclear charge. (correct)
- Remains constant as the number of electron shells stays the same.
Ionization energy generally decreases as you move down a group in the periodic table.
Ionization energy generally decreases as you move down a group in the periodic table.
True (A)
What is the definition of electronegativity?
What is the definition of electronegativity?
Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons.
The energy released when an electron is added to a neutral atom is known as ______.
The energy released when an electron is added to a neutral atom is known as ______.
Match each element with its expected metallic character.
Match each element with its expected metallic character.
Which element has the highest electronegativity?
Which element has the highest electronegativity?
Elements with high ionization energies tend to readily lose electrons.
Elements with high ionization energies tend to readily lose electrons.
Name two elements that are considered to be in the Halogen Family.
Name two elements that are considered to be in the Halogen Family.
The ______ are located in group VIIIA, and are known for being inert due to their full valence shell
The ______ are located in group VIIIA, and are known for being inert due to their full valence shell
Match the element with the Family Group.
Match the element with the Family Group.
As you move across the periodic table from left to right, what generally happens to the metallic character of the elements?
As you move across the periodic table from left to right, what generally happens to the metallic character of the elements?
Atomic radius is defined as the distance between the nucleus and the closest electron.
Atomic radius is defined as the distance between the nucleus and the closest electron.
Briefly explain why ionization energy increases across a period.
Briefly explain why ionization energy increases across a period.
Elements in the same ______ of the periodic table exhibit similar chemical properties.
Elements in the same ______ of the periodic table exhibit similar chemical properties.
Match the following elements with their electron configurations.
Match the following elements with their electron configurations.
Which of the following elements is most likely to have the highest electron affinity?
Which of the following elements is most likely to have the highest electron affinity?
Electronegativity generally increases down a group in the periodic table.
Electronegativity generally increases down a group in the periodic table.
How does the metallic character of an element relate to its ability to lose electrons?
How does the metallic character of an element relate to its ability to lose electrons?
The trend in periodic properties is primarily due to changes in effective nuclear ______ and electron configuration.
The trend in periodic properties is primarily due to changes in effective nuclear ______ and electron configuration.
Match the following elements with their general periodic trend properties.
Match the following elements with their general periodic trend properties.
Which factor primarily influences the trend in ionization energy across a period?
Which factor primarily influences the trend in ionization energy across a period?
Nonmetals generally have lower electronegativity values compared to metals.
Nonmetals generally have lower electronegativity values compared to metals.
Explain the concept of 'shielding' and its effect on ionization energy.
Explain the concept of 'shielding' and its effect on ionization energy.
Moving down a group, the addition of electron ______ increases the atomic radius.
Moving down a group, the addition of electron ______ increases the atomic radius.
Match each element with its likely ionic charge based on its group in the periodic table.
Match each element with its likely ionic charge based on its group in the periodic table.
Which of the following best explains why atomic radius increases down a group in the periodic table?
Which of the following best explains why atomic radius increases down a group in the periodic table?
Elements with high metallic character tend to have high ionization energies.
Elements with high metallic character tend to have high ionization energies.
Explain the difference between atomic radius and ionic radius.
Explain the difference between atomic radius and ionic radius.
The electron affinity of noble gases is typically close to ______.
The electron affinity of noble gases is typically close to ______.
Match the following terms with their descriptions.
Match the following terms with their descriptions.
Which property is generally associated with nonmetals?
Which property is generally associated with nonmetals?
The atomic radius of a cation is larger than its corresponding neutral atom.
The atomic radius of a cation is larger than its corresponding neutral atom.
Describe the trend in metallic character as you move down Group 1A (the alkali metals).
Describe the trend in metallic character as you move down Group 1A (the alkali metals).
Elements with similar valence electron configurations and chemical properties are grouped into ______.
Elements with similar valence electron configurations and chemical properties are grouped into ______.
Match each description with the appropriate periodic trend.
Match each description with the appropriate periodic trend.
Which of the following electron configurations represents an element with the lowest ionization energy?
Which of the following electron configurations represents an element with the lowest ionization energy?
Elements in the same period have similar chemical properties.
Elements in the same period have similar chemical properties.
How does increasing effective nuclear charge affect electron affinity?
How does increasing effective nuclear charge affect electron affinity?
The element with the electron configuration of 1s² 2s²2p² would be in whch family group? ______
The element with the electron configuration of 1s² 2s²2p² would be in whch family group? ______
Match the following properties with the family group that is most strongly associated with that property.
Match the following properties with the family group that is most strongly associated with that property.
Flashcards
Periodic Trends
Periodic Trends
Specific patterns that illustrate different aspects of elements on the periodic table.
Atomic Radius
Atomic Radius
The distance from the center of the nucleus to the outermost electron shell.
Ionic Radius
Ionic Radius
The distance between the nucleus and the electron in the outermost shell of an ion.
Metallic Property
Metallic Property
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Ionization Energy
Ionization Energy
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Electron Affinity
Electron Affinity
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Electronegativity
Electronegativity
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Study Notes
- Periodic trends are specific patterns present in the periodic table.
- The trends illustrate varying aspects of elements.
Common Periodic Trends
- Atomic Radius
- Metallic Property
- Ionization Energy
- Electron Affinity
- Electronegativity
Atomic Radius
- Atomic radius measures the distance from the center of the nucleus to the outermost electron shell.
- Ionic radius measures the distance between the nucleus and the electron in the outermost shell of an ion.
- An anion is negative, while a cation is positive.
Metallic Property
- Metallic property refers to an atom's ability to donate electrons.
Ionization Energy
- Ionization energy is the energy needed to remove an electron from its orbital around an atom.
Electron Affinity
- Electron affinity is the energy released when an electron is added to a neutral atom in the gaseous state.
- Higher electron affinity means a greater attraction for an electron.
Electronegativity
- Electronegativity measures the tendency of an atom to attract a bonding pair of electrons.
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