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Back to AI Flashcard MakerBiochemistry /Atomic Structure and Periodic Properties Part 1

Atomic Structure and Periodic Properties Part 1

Biochemistry35 CardsCreated 4 months ago

This deck covers fundamental concepts of atomic structure and periodic properties, including electron configurations, periodic trends, and characteristics of elements.

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What are periodic properties?

Properties whose values can be predicted based on the element's position on the periodic table
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Key Terms

Term
Definition
What are periodic properties?
Properties whose values can be predicted based on the element's position on the periodic table
What is the basis for the transmission of nerve signals?
Movement of ions across cell membranes
In what directions are Na+ and K+ ions pumped across membranes through ion channels?
Na+ moves OUT K+ moves IN
How do we represent orbitals?
Represented as a square and the electrons in that orbital as arrows. The direction of the arrow represents the spin of the electron
What is electron configuration?
Describes how the electrons are distributed in the various atomic orbitals.
What is the Pauli exclusion principle?
No two electrons in an atom can have the same four quantum numbers
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Atomic Structure and Periodic Properties Part 1
TermDefinition
What are periodic properties?
Properties whose values can be predicted based on the element's position on the periodic table
What is the basis for the transmission of nerve signals?
Movement of ions across cell membranes
In what directions are Na+ and K+ ions pumped across membranes through ion channels?
Na+ moves OUT K+ moves IN
How do we represent orbitals?
Represented as a square and the electrons in that orbital as arrows. The direction of the arrow represents the spin of the electron
What is electron configuration?
Describes how the electrons are distributed in the various atomic orbitals.
What is the Pauli exclusion principle?
No two electrons in an atom can have the same four quantum numbers
What does each electron in a multielectron atom experience?
Both the attraction to the nucleus and the repulsion by other electrons in the atom.
What is the effective nuclear charge?
Total amount of attraction that an electron feels for the nucleus
What happens when the electrons are closer to the nucleus?
The more attraction it experiences
The better an outer electron is at penetrating through the electron cloud of inner electrons...
The more attraction it will have for the nucleus
What is the Aufbau Principle?
States that electrons are added to the lowest energy orbitals first before moving to higher energy orbitals
What is Hund's rule?
The most stable arrangement of electrons is the one in which the number of electrons with the same spin is maximized Put one electron in each before pairing.
What are the general rules for writing electron configurations?
1. Electrons will reside in the available orbitals of the lowest possible energy 2. Each orbital can accommodate a maximum of two electrons. 3. Electrons will not pair in degenerate orbitals if an empty orbital is available 4. Orbitals will fill in the order indicated in the figure.
How can electron configurations of all elements except hydrogen and helium be represented?
Noble gas core
What are the valence electrons?
The outermost electrons of an atom
What are core electrons?
Electrons in lower energy shells.
What are the main group elements? (representative elements)
Elements in Groups 1A through 7A
What group are the noble gases?
Group 8A Have completely filled p sub shells.
What group are the transition metals?
Groups 3-12
What make up the f-block transition elements?
Lanthanides and actinides
What is the effective nuclear charge (Z-eff) -lecture 2?
The actual magnitude of positive charge that is "experienced" by an electron in the atom.
How does the value of the effective nuclear charge increase?
Increases steadily from left to right
What is the atomic radius?
Distance between the nucleus of an atom and its valence shell
How does the atomic radius increase?
Increases from top to bottom down a group. Increasing n, so outermost shell lies farther from the nucleus.
How does the atomic radius decrease?
Left to right across a period Increasing Z-eff which draws the valence shell closer to the nucleus
What is the ionization energy (IE)?
Minimum energy required to remove an electron from an atom in the gas phase. Results in an ion, a chemical species with a net charge. Na(g)-->Na+ (g) + e-
What happens to the ionization energy as the Z-eff increases?
Ionization energy increases IE increases from left to right across a period.
Why is removing a paired electron easier?
Because of the repulsive forces between two electrons
Why does it take more energy to remove the second, third, fourth, and so on electrons?
Harder to remove an electron from a cation than an atom. Takes more energy to remove core electrons than valence. Core electrons are closer to nucleus
What is electron affinity (EA)?
Negative of the energy released when an atom in the gas phase accepts an electron Cl(g)+e- ---> Cl- (g)
How does electron affinity increase?
Like ionization energy Increases from left to right across a period as effective nuclear charge increases. Easier to add an electron as the positive charge of the nucleus increases.
Is it easier to add an electron to an s orbital than to add one to a p orbital with the same quantum number?
YES
Characteristics of metals:
CATIONS Shiny Malleable Ductile Good conductors of both heat and electricity Low ionization energies Commonly form cations
Characteristics of nonmetals:
ANIONS Vary in color Not shiny Brittle Poor conductors of heat and electricity High electron affinities Form anions
Characteristics of metalloids:
Elements with properties intermediate between those of metals and nonmetals.