PHA615 LEC: Covalent Bonding and Shape of Molecules

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Organic chemistry

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is the branch of chemistry that deals with the chemistry of living “organic” substances (e.g. substances from animals and plant)s

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Inorganic Chemistry

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INORG OR ORG?

It is the general study of chemicals / elements.

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71 Terms

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Organic chemistry

is the branch of chemistry that deals with the chemistry of living “organic” substances (e.g. substances from animals and plant)s

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Inorganic Chemistry

INORG OR ORG?

It is the general study of chemicals / elements.

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Inorganic Chemistry

INORG OR ORG?

Minerals

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Inorganic Chemistry

INORG OR ORG?

All elements in the periodic table

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Organic Chemistry

INORG OR ORG?

It is specific to the study of CARBON and to all substances containing it.

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Organic Chemistry

INORG OR ORG?

Biological species (animals, plants)

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Organic Chemistry

INORG OR ORG?

C, H, O, N, S, P, X (halogens)

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hydrocarbons

composed entirely of C and H atoms

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hydrocarbon derivatives

composed of C, H, and one or more element.

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4

Carbon atoms based on their atomic configuration will have _ valence electron and must form _ bonds to achieve its Octet rule.

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Atomic number

gives the # of protons / electrons

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Mass number

the total # of protons and neutrons in the nucleus.

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Atomic Orbitals

  • Also known as wave function.

  • It is the solution to a wave equation — the mathematical expression used to describe the distribution of electrons in an atom.

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spherical

shape of s orbital

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dumbbell shape

shape of p orbital

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ORBITAL

a region of space around a nucleus where electrons are most likely to be found.

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electron shells

Atomic orbitals are arranged around the nucleus in different layers known as “__” based on their sizes and energy levels.

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Hund’s principle

states that every orbital in a subshell is singly occupied before other orbitals are completely filled and that electrons in a singly occupied orbital will have the same spin

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Aufbau’s principle

states that electrons will fill the lowest available energy level before filling the higher levels

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Pauli’s Exclusion principle

states that no two electrons will have identical quantum numbers (spin is opposite)

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Octet rule

states that the valence shell (outermost shell) must be filled completely and must achieve a noble gas configuration (8 valence electron).

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Ionic Bond

IONIC OR COVALENT

Electrons are transferred.

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Ionic Bond

IONIC OR COVALENT

Between atoms of different eletronegativity (cations and anions)

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Ionic Bond

IONIC OR COVALENT

Metals and Non-metals

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Covalent Bond

IONIC OR COVALENT

Electrons are shared.

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Covalent Bond

IONIC OR COVALENT

Between similar atoms and atoms of nearly equal electronegativity.

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Covalent Bond

IONIC OR COVALENT

Non-metals

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Lewis dot structure

shows the kernel or nucleus represented by the symbol of the atom surrounded by its valence electrons represented by dots.

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Kekule structure

also known as line-bond structures; shows 2- electron covalent bonds as a line and the lone-pair electrons (non-bonding electrons) as dots.

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Electronegativity

a measure of the relative attraction an atoms has for the shared electron in a bond.

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Bond polarity

a measure of the degree of inequality in the sharing of electrons between two atoms in a chemical bond.

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Non-polar covalent bond

a covalent bond in which there is a equal sharing of electrons between two atoms.

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Polar covalent bond

a covalent bond in which there is an unequal sharing of electrons between two atoms.

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2 and above

Electronegative difference of Ionic bonds

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1.5-2

Electronegative difference of ionic or polar covalent

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1.5-0.4

Electronegative difference of polar covalent

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0.4 and below

Electronegative difference of nonpolar covalent

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Formal Charge

the no. of valence electrons in the neutral atom minus the number of covalent bonds to the atom and the number of unshared electrons on the atom.

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Formal Charge

these charges will have an impact on chemical reactions and product formation.

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Orbital hybridization

is a concept of combining orbitals to form hybrid orbitals that are suitable for pairing electrons to form covalent bonds.

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Tetrahedral,

the geometric shape of carbon with 4 hybridize orbitals with a specific bond angle.

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sigma bonds

  • head-on overlap

  • stronger

  • hybrid

  • sp3

  • single bond

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pi bond

  • sideway overlap

  • weaker (reactive)

  • unhybrid

  • sp2 and sp

  • found in double or triple bond (BELOW in double; top and bottom in triple)

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sp3 carbon

forms when 2s orbital hybridize with 3 2p orbitals forming four (4) sp3 hybrid orbitals.

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sp2 carbon

forms when 2s orbital hybridize with 2 2p orbitals forming three (3) sp2 hybrid orbitals and one (1) unhybridized p-orbital.

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sp carbon

forms when 2s orbital hybridize with 1 2p orbital forming two (2) sp hybrid orbitals and two (2) unhybridized p-orbitals.

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Functional Group

  • a group of atom within a molecule that possess a characteristic behavior.

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Functional Group

  • is a structural feature of a molecule which determine its reactivity and can therefore be used for molecule classification.

  • moiety or portion of the structure that undergoes specific reactions.

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Linear

a straight-chain molecule with no branching substituents.

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Branched

a straight chain of atoms, usually carbon, with any number of secondary, straight-chain branches.

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Cyclic

a compound in which a series of atoms are connected to form a ring.

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Saturated organic molecule

is composed of all sp3 hybridized carbons.

All carbons form only single bonds with each other (e.g. Alkane)

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Unsaturated organic molecule

possesses a number of pi-bond (1 or 2)

which allows further addition of new atoms into the chain (e.g. alkene / alkyne).

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Addition

the combination of two or more molecules to form a bigger molecule.

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Elimination

a reaction wherein two substituents are removed from a molecule either in one-step or two-step mechanism.

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Substitution

a reaction wherein one functional group in a compound is replaced by another functional group.

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Rearrangement

a reaction wherein the carbon skeleton of an organic molecule is rearranged to yield a structural isomer of the original molecule (mostly for stability purposes).

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Organic REDOX

oxidation or reduction reactions of some functional groups in an organic molecule.

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Addition

halogenation,

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Addition

hydrogenation,

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Addition

hydrohalogenation

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Addition

acetal formation

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Addition

hydrate formation

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Elimination

dehydration

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Elimination

Unimolecular or Bimolecular elimination (E1/E2)

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Substitution

Types: Aromatic Electrophilic (SE), Radical

(SR), Unimolecular or Bimolecular Nucleophilic (SN1/SN2),

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Substitution

Nucleophilic aliphatic/acyl

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Substitution

Friedel-Craft’s Acylation and Alkylation

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Rearrangement

tautomerization,

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Rearrangement

hydride/methide shift

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bonding electrons

number of electrons - number of valence electrons