INTRO TO ORGCHEM : Structure And Bonding Flashcards by Aliyah Dela Cruz

Study of carbon and carbon-related compounds.

Organic Chemistry

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The name “organic chemistry” comes from the word?

Organism

(Because most of the organic compounds were isolated or obtained from organisms or their remains)

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In year ____ , ______, a German Chemist, disproved the “Vitalism theory which states that all organic compounds come from living things. He was able to isolate ______ from an inorganic compound, __________.

• 1828
• Friedrich Wohler
• urea
• ammonium cyanate

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What are the organic compounds found in living things?

Sugars
Lipids
Proteins
Nucleic Acids

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A polymer made up of units called nucleotides.

DNA

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What are the three different components that made up nucleotides?

Sugar group
Phosphate group
Base

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What are the 4 different bases?

Adenine
Thymine
Guanine
Cytosine

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What holds DNA strands together?

Hydrogen bonds (between bases on adjacent strands)

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______ compounds usually do not dissolve in water.

Organic

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______ compounds usually dissolve in water.

Inorganic

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_____ compounds generally dissolve in organic solvents like ether, alcohol, benzene, and choloroform.

Organic

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_______ compounds generally do not dissolve in organic solvents.

Inorganic

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_______ compounds have usually low melting points and boiling points; and they usually decompose on heating.

Organic

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_______ compounds usually have high melting points and boiling points. They usually do not decompose on heating.

Inorganic

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_______ compounds are inflammable; they catch fire easily.

Organic

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_______ compounds are usually non inflammable; they do not burn easily.

Inorganic

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_______ compounds exist as covalent molecules, so they are non-electrolytes.

Organic

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Most of the _______ compounds are ionic, so they are electrolytes.

Inorganic

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Carbon is able to form how many covalent bonds?

4 covalent bonds

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What atoms have the ability to bond to each other to form long chains or rings?

Carbon atoms

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What atoms link together to form chains of varying lengths, branched chains and rings of different sizes?

Carbon atoms

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Smallest particle of an element

Atoms

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Neutral subatomic particle

Neutron

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Positively charged subatomic particle (+1 charge)

Proton

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Negatively charged subatomic particle (-1 charge)

Electron

Center of an atom; contains protons and neutrons

Nucleus

Consists of a nucleus surrounded by electrons that are equal in number to the protons of the nucleus.

Atom

Atoms of the same element with different numbers of neutrons and thus different mass number.

Isotopes

Carbon-12 (stable isotope)

98.9% 6 protons & 6 neutrons

Carbon-13 (stable isotope)

1.1% 6 protons & 7 neutrons

Carbon-14 (unstable isotope; radioactive)

<0.1% 6 protons & 8 neutrons

Fundamental building blocks of all substances.

Elements

- Region of space where there is a certain probability of finding an electron - Can hold 2 electrons - Also known as WAVE FUNCTION

Orbitals

Shape of s orbital

Spherical

Shape of p orbital

Dumbbell

Shape of d orbital

4 leaf clover

Shape of f orbital

Complex shape

States that electron fill lower-energy atomic orbitals before filling higher-energy ones.

Aufbau Principle

Maximum of 2 electrons can occupy thr same orbital only if they have opposite spins.

Pauli's Exclusion Principle

For degenerate orbitals, electrons fill the orbitald singly before they pair up.

Hund's Rule

Determine the size of the particle.

Principal Quantum Number

Subshell or sublevel, determines the shape

Azimuthal or Angular Momentum

Orbitals, determines orientation

Magnetic

Direction of spin or orientation

Spin

- Symbolic notation of the manner in which the electrons of its atoms are distributed over different atomic orbitals. - Summary of where the electrons are around a nucleus

Electron Configuration

Number of negatively charged subatomic particles in the highest energy level of atoms that enters into formation of chemical bonds.

Valence Electrons

- joining of two atoms in a stable arrangement - may occur between atoms of the same or different elements. - favorable process because it always leads to lowered energy and increased stability - octet rule - atoms react in a way that achieve valence shell of eight valence electrons.

Chemical Bonding

- bond between cation and anion - atom may lose or gain enough electrons to acquire a completely filled valence shell - anions gain electrons; cations lose electrons

Ionic Bond

Sharing of electrons

Covalent Bond

- electron dot structure - valence shell electrons of an atom are represented as dot

Lewis Structure

- line bond structure - each shared electron is represented by line between the atom symbols

Kekule Structure

Pair of valence electrons that are not used for bonding.

Lone-pair electrons / non-bonding electrons

Associated with any atom that does not exhibit the appropriate number of valence electrons.

Formal Charge

Measure of the ability of an atom to attract electrons.

Electronegativity

Seperation of electric charge along a bond, leading to a molecule or its chemical groups having an electric dipole or dipole moment

Bond polarity

Formula of formal charge

# of valence electrons - sum between non bonded electrons + # of line bonds

Most electronegative element

Fluorine

Equally shared electrons between the atoms. (Difference in electronegativity < 0.5

Non-polar covalent bond

Not equally shared electrons between atoms. (0.5 - 1.7 electronegativity)

Polar covalent bond

Withdrawal of electrons towards a highly electronegative atom which causes the formation of partial charges.

Induction

Average out energy

sp³ hybridization

Å is?

(Angstrom) - Unit for length

- total number of sigma bonds and lone pairs - indicated the number of electron pairs (bonding and non-bonding) that are repelling each other.

Steric number

How to get steric number?

# of bonds + # of lone pairs

Bond angle: 107 degrees - e.g. ammonia

Trigonal pyramidal

Bond angle: 105

Bent

Bond angle: 120 degrees - e.g. Boron trifluoride

Trigonal planar

subshell is known as?

atomic orbitals

Equally shared electrons between 2 atoms

Non-polar covalent bond

Not equally shared electrons between atoms

Polar covalent bond

Is < 0.5 polar or non-polar?

Non-polar covalent bond

Is 0.5 - 1.7 polar or non-polar?

Polar covalent bond

If the central atom is connected to the same groups/atoms (symmetrical) (Non-Polar or Polar)

Non-Polar

It has no lone pair (in the central atom) (Non-Polar or Polar)

Non-Polar

If the central atom is connected to different groups/atoms (asymmetrical) (Non-Polar or Polar)

Polar

If it has a lone pair (in the central atom) (Non-Polar or Polar)

Polar