Structure and Bonding Flashcards by MICHAEL JOSH SAN FELIPE

protons and neutrons
electron cloud
mass (nucleus)
volume (electron)

Atomic Structure

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two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons

Isotopes

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electron location unknown but electron density is known

Quantum Mechanical Model

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electron will be in a certain region of space (orbital) at a given instant

Electron Density

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Electrons do not circle around the nucleus in fixed orbits but rather,
in ________.

Orbitals

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Each orbital has a characteristic _____and ____ (energy).

Shape and Size

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used to described orbitals

Quantum Numbers

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lowest-energy orbitals fill up first

Aufbau Principle

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If two or more empty orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half-full,

Hund’s Rule

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Only two electrons can occupy an orbital, and they must
have opposite spins

Pauli’ Exclusion Principle

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there is a limit to the precision with which certain pairs of physical properties can be simultaneously known

Heisenberg’s Uncertainty Principle

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Electron BELOW the outermost shell

Core Electrons

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Electrons IN the outermost shell

Valence Electrons

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An attractive force between two ions or between two atoms

Chemical bond

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Why do chemical bonds form?

more stable and lower in energy

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How do chemical bonds form?

Octet Rule

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Chemistry of main-group elements is governed by their tendency to
take on the electron configuration of the nearest noble gas.

Octet Rule

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Attractive forces between opposite charges

Electrostatic Attraction

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formed in electrostatic attraction
formed in transfer of electrons
reaction of metals with nonmetals

Ionic Bond

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Compounds formed by ionic bonds

Ionic Compound

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Bond formed as a result of sharing electrons between two nuclei

Covalent Bond

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Compounds formed by covalent bonds

Molecular compounds

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Measure of the ability of an atom to pull the bonding electrons toward itself

Electronegativity

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covalent bond between atoms with SAME electronegativity

Nonpolar covalent bond

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covalent bond between atoms with DIFFERENT ELECTRONEGATIVITIES

Polar covalent bond

< 0.4

pure covalent

between 0.4 and 1.8

Polar covalent

> 1.8

ionic

a pair of equal and oppositely charged poles separated by a DISTANCE

Dipole

Measure of Dipole

Dipole moment

magnitude of the charge on either atom x distance between the two charges

Dipole moment

electron-dot structures

Lewis Structures

line-bond structures

Kekule Structures

not an actual charge, used for bookkeeping of electrons

Formal charge

charge if each bonding electron pair in the molecule were shared equally between atoms

Formal Charge

Difference VE when it is not bonded and VE when it is bonded

Formal Charge

OMITTING OF THE COVALENT bonds and listing atoms bonded to a particular carbon (or nitrogen or oxygen) next toit (with a subscript if there is more than one of a particular atom)

Condensed structures

C atoms aren't shown C atoms are assume in the lines H atoms aren't shown Atoms other than C and H are shown

Skeletal structures

Shows 3D shape

Perspective Drawing

Show bond angles accurately

Ball-and-Stick Model

Shows atoms in scale

Space-filling Model

Bond lies in the plane of the paper

Normal Bond

Bond extends backwards, away from the viewer

Dashed bond

Bond protudes forwards, toward the viewer

Wedged bond

Geometry based on arrangement of atoms in a molecule + defined by bond angles

Molecular Geometry

Geometry based on valence electron pairs around a central atom + Defined by bond angles

Electron pair geometry

A model for the prediction of molecular geometry based on the MINIMIZATION OF ELECTRON REPULSION between regions of eelctron density around an atom

Valence-Shell Electron-Pair Repulsion Model (VSEPR)

The best arrangement of a given number of electron pairs (bonding and nonbonding) is the one that minimizes the repulsions among them.

Valence-Shell Electron-Pair Repulsion Model (VSEPR)

Without lone pairs:

Electron Pair Geometry and Molecular Geometry is equal

assumes that the electrons in a molecule occupy OVERLAPPING atomic orbitals of the individual atoms

Valence Bond Theory

Assumes the formation of molecular orbitals from the atomic orbitals

Molecular Orbital Theory

How is covalent bonds formed?

When atomic orbitals on neighboring atoms overlap one another

head-on overlap of atomic orbitals; stronger

Sigma σ

sideway overlap of atomic orbitals; weaker

PI BONDS (π)

atomic orbitals obtained when TWO OR MORE NONEQUIVALENT ORBITALS of the SAME ATOM combine for covalent bond formation

Hybrid Orbitals

Produces the molecular geometry of the molecule.

Hybridization

The greater the electron density in the gregion of orbital overlap

The stronger and shorter the bond

As s character increases, bond angle _______

Increases

Describes a region of space in a molecule where electrons are most likely to be found

Molecular Orbital

2 ways to combine atomic orbitals into molecular orbitals

Additive and Subtractive

2 ways to combine atomic orbitals into molecular orbitals ? - Lower energy, bonding molecular oribtal

Additive

2 ways to combine atomic orbitals into molecular orbitals ? - higher energy, antibonding molecular orbital

Subtractive

occurs when an electron is shared by more than 2 atoms with π bonds (p orbitals)

π ELECTRON DELOCALIZATION

Structures are represented by resonance contributors

π ELECTRON DELOCALIZATION

Some substances can’t be represented by a single line-bond structure and must be considered as a resonance hybrid of two or more structures.

Resonance

two individual line-bond structures

Resonance forms

indicated by the double- headed arrow between them.

Special Resonance Relationship

What is the different between resonance forms?

Placement of the π BOND and NONBONDING VALENCE ELECTRONS

single unchanging structure

Resonance Hybrid

two individual forms and has characteristics of both

Resonance Hybrid

Between resonance forms

Double headed arrow

Movement of electrons

Curly Arrow

From electron-rich species

Tail

To electron-deficient specials

Head

Double bonds separated by single bonds

Conjugation

Refers to a system that has a p orbital adjacent to a π bond allowing delocalization of π electrons

Conjugation

Compounds with isolated double bonds (___________)

Higher energy

Special kind of conjugation and cyclic unsaturated molecules with unusual stability

Aromaticity

Originally used to classify benzene and its derivatives because many of them have distinctive odors

Aromaticity

Structure and Bonding Flashcards

Definitions (80 cards)