Podcast
Questions and Answers
What is the best way to show the chemical reactivity of an element?
What is the best way to show the chemical reactivity of an element?
By its reactions with oxygen and halogens
Which elements in a period combine easily with oxygen?
Which elements in a period combine easily with oxygen?
Elements on the two extremes of a period
What is the nature of the oxide formed by the element on the extreme left of a period?
What is the nature of the oxide formed by the element on the extreme left of a period?
Basic
What is the nature of the oxide formed by the element on the extreme right of a period?
What is the nature of the oxide formed by the element on the extreme right of a period?
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What is the nature of oxides of elements in the centre of a period?
What is the nature of oxides of elements in the centre of a period?
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How do amphoteric oxides behave?
How do amphoteric oxides behave?
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What is the relationship between electronic configuration and periodic trends?
What is the relationship between electronic configuration and periodic trends?
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What is the general trend in atomic and ionic radii in a period?
What is the general trend in atomic and ionic radii in a period?
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What is the significance of electron configuration in understanding chemical reactivity?
What is the significance of electron configuration in understanding chemical reactivity?
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Why do elements on the two extremes of a period react with oxygen?
Why do elements on the two extremes of a period react with oxygen?
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Study Notes
Atomic Radius
- The distance between two adjacent copper atoms in solid copper is 256 pm, so the metallic radius of copper is 128 pm.
- Atomic radius increases as the atom size increases, reflected in atomic radii.
- Note that atomic radii of noble gases are not considered, and their values are very large.
Periodic Table and Electronic Configurations
- The element's location in the Periodic Table reflects the quantum numbers of the last orbital filled.
- The period indicates the value of n for the outermost or valence shell.
- Successive periods in the Periodic Table are associated with the filling of the next higher principal energy level (n = 1, n = 2, etc.).
- The sixth period (n = 6) contains 32 elements, and successive electrons enter 6s, 4f, 5d, and 6p orbitals in that order.
- The seventh period (n = 7) is similar to the sixth period, with the successive filling of the 7s, 5f, 6d, and 7p orbitals.
Ionization Enthalpy
- Ionization enthalpy increases across a period due to the increasing nuclear charge, which outweighs the shielding effect.
- The effective nuclear charge experienced by a valence electron is less than the actual charge on the nucleus due to shielding.
- Shielding is effective when the orbitals in the inner shells are completely filled, as seen in the case of alkali metals.
- The first ionization enthalpy of an element is influenced by the shielding effect and the electron-electron repulsion.
Periodic Trends and Chemical Reactivity
- Atomic and ionic radii, ionization enthalpy, electron gain enthalpy, and valence are all related to electronic configuration.
- The periodicity is related to electronic configuration, and all chemical and physical properties are a manifestation of this.
- Elements on the extremes of a period easily combine with oxygen to form oxides, with the most basic oxide formed by the element on the extreme left and the most acidic oxide formed by the element on the extreme right.
- Oxides of elements in the centre are amphoteric or neutral.
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Description
This quiz is about the atomic radius of copper, its measurement and how it relates to the size of atoms. It also touches on the concept of metallic radius and atomic radii of noble gases.
