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Questions and Answers
What is the main focus of Module-1: PERIODIC PROPERTIES?
What property is associated with the tendency of an atom to attract a bonding pair of electrons?
Which factor determines the size of an atom in the periodic table?
What is the measure of the ease with which an atom can lose an electron?
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What is the effective nuclear charge experienced by an electron in a multi-electron atom?
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What determines the variation of s, p, d, and f orbital energies of atoms in the periodic table?
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What is the main factor contributing to the trend of increasing ionization energy across a period in the periodic table?
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What property of an atom refers to its ability to attract an additional electron to form a negative ion?
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What factor primarily influences the size of an atom in the periodic table?
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What is the measure of the ability of an atom to attract a bonding pair of electrons?
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What primarily influences the size of an atom in the periodic table?
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What is the main factor contributing to the trend of increasing ionization energy across a period in the periodic table?
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Which property of an atom refers to its ability to attract an additional electron to form a negative ion?
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What determines the variation of s, p, d, and f orbital energies of atoms in the periodic table?
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Study Notes
Main Focus of Module-1: PERIODIC PROPERTIES
- Explores the trends and patterns in elemental properties within the periodic table.
- Analyzes periodic trends such as atomic size, ionization energy, electronegativity, and electron affinity.
Tendency to Attract Bonding Electrons
- The property associated with an atom's tendency to attract a bonding pair of electrons is known as electronegativity.
Atom Size Determination
- The size of an atom is primarily determined by atomic radius, which is influenced by the number of electron shells and the effective nuclear charge.
Ease of Electron Loss
- The measure of how easily an atom can lose an electron is called ionization energy.
Effective Nuclear Charge in Multi-Electron Atoms
- Effective nuclear charge refers to the net positive charge experienced by an electron in a multi-electron atom, accounting for both the protons in the nucleus and the shielding effect of other electrons.
Orbital Energy Variation
- The variation in s, p, d, and f orbital energies is determined by electron-electron interactions and the differences in the principal quantum number alongside the shape of the orbitals.
Increasing Ionization Energy Trend
- The trend of increasing ionization energy across a period is mainly due to increasing effective nuclear charge, which pulls electrons closer to the nucleus.
Ability to Form Negative Ions
- The property of an atom that indicates its ability to attract an additional electron to form a negative ion is known as electron affinity.
Influence on Atom Size
- Factors influencing atomic size include nuclear charge, the number of electron shells, and the shielding effect caused by inner electrons.
Measure of Electron Pair Attraction
- The ability of an atom to attract a bonding pair of electrons is quantified by its electronegativity.
Repeated Factors Influencing Atom Size
- Again, the primary influences on atomic size are nuclear charge, the number of electron shells, and electron shielding.
Trend in Ionization Energy
- The increasing ionization energy across a period is again linked to effective nuclear charge, reinforcing the pull on the outer electrons.
Ability to Attract Additional Electrons
- An atom's ability to attract an extra electron, forming a negative ion, is defined by its electron affinity.
Determinants of Orbital Energies
- Orbital energy variations in the periodic table are influenced by nuclear charge, electron configuration, and the degree of electron shielding in various sublevels.
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Description
Test your knowledge of periodic properties with this quiz based on Dr. Puspanjali Mishra's syllabus. Explore topics such as effective nuclear charge, orbital energies, atomic sizes, ionization energies, and more. Perfect for chemistry students and enthusiasts.
