Podcast
Questions and Answers
How does the shielding effect influence the ionization energy of an atom?
How does the shielding effect influence the ionization energy of an atom?
- Decreases ionization energy by reducing the effective nuclear charge experienced by outer electrons. (correct)
- Has no effect on ionization energy.
- Increases ionization energy by strengthening the attraction between the nucleus and outer electrons.
- Shielding effect directly equals ionization energy.
Which of the following statements correctly describes the trend in atomic radius as you move down Group 1 (alkali metals) on the periodic table?
Which of the following statements correctly describes the trend in atomic radius as you move down Group 1 (alkali metals) on the periodic table?
- Atomic radius remains constant.
- Atomic radius decreases due to increasing nuclear charge.
- Atomic radius increases due to the addition of electron shells. (correct)
- Atomic radius decreases due to effective nuclear charge.
Considering the trends in electronegativity, which of the following pairs of elements would form the most polar bond?
Considering the trends in electronegativity, which of the following pairs of elements would form the most polar bond?
- Carbon (C) and Hydrogen (H)
- Silicon (Si) and Oxygen (O)
- Magnesium (Mg) and Sulfur (S)
- Sodium (Na) and Chlorine (Cl) (correct)
How does the trend in metallic character generally vary across the periodic table?
How does the trend in metallic character generally vary across the periodic table?
What is ionization energy and how does it generally trend across a period (from left to right) on the periodic table?
What is ionization energy and how does it generally trend across a period (from left to right) on the periodic table?
How does adding an electron to an atom typically affect its size, and what is the resulting ion called?
How does adding an electron to an atom typically affect its size, and what is the resulting ion called?
In terms of electron affinity, which of the following elements is most likely to release the greatest amount of energy when gaining an electron?
In terms of electron affinity, which of the following elements is most likely to release the greatest amount of energy when gaining an electron?
Considering their positions on the periodic table, which element is expected to have the highest electronegativity?
Considering their positions on the periodic table, which element is expected to have the highest electronegativity?
Which factor is most responsible for the increase in atomic size as you move down a group in the periodic table?
Which factor is most responsible for the increase in atomic size as you move down a group in the periodic table?
Predict the element with the lowest first ionization energy from the list below:
Predict the element with the lowest first ionization energy from the list below:
How does the 'looseness' of valence electrons relate to the metallic properties of an element?
How does the 'looseness' of valence electrons relate to the metallic properties of an element?
Which of the following best explains why noble gases are generally unreactive?
Which of the following best explains why noble gases are generally unreactive?
If element X forms a stable ion with a 2+ charge, and it's located in the same period as Potassium (K), what can be inferred about element X?
If element X forms a stable ion with a 2+ charge, and it's located in the same period as Potassium (K), what can be inferred about element X?
Considering the positions of Oxygen (O) and Sulfur (S) on the periodic table, which statement accurately compares their electron affinities?
Considering the positions of Oxygen (O) and Sulfur (S) on the periodic table, which statement accurately compares their electron affinities?
How would you describe the relationship between atomic radius and ionization energy trends across a period?
How would you describe the relationship between atomic radius and ionization energy trends across a period?
Flashcards
Atomic Radius
Atomic Radius
Distance from the nucleus of an atom to its outermost orbital.
Shielding Effect
Shielding Effect
The effect where inner electrons shield outer electrons from the full positive charge of the nucleus.
Ionization Energy
Ionization Energy
Energy required to remove the outermost electron from an atom.
Electronegativity
Electronegativity
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Electron Affinity
Electron Affinity
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Metallic Property
Metallic Property
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Ionic Size
Ionic Size
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Study Notes
- Properties of elements can be predicted from their arrangement on the periodic table.
Atom Size/Atomic Radius
- Atomic radius refers to the distance from the nucleus of an atom to its outermost orbital.
- Atomic size increases down a group.
- Atomic size decreases across a period from left to right.
Shielding Effect
- Shielding effect is the attraction between the nucleus and outer electrons, and the repulsion between inner electrons.
Ionization Energy
- Ionization energy is the energy required to remove the outermost electron from an atom.
Electronegativity
- Electronegativity is the ability of an atom to attract electrons to itself.
Electron Affinity
- Electron affinity is the energy change when an electron is added to an atom and describes the attraction of the nucleus to the electrons.
Metallic Property
- Metallic property refers to the looseness of valence electrons of an atom.
Ionic Size
- Ionic size is the size of an atom when it gains an electron (anion) or loses an electron (cation).
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