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Orgchem > Organic Compounds and Functional Groups > Flashcards

Organic Compounds and Functional Groups Flashcards

1
Q

contain the element carbon

A

Organic Chemistry

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2
Q

What are the 2 that organic compounds formerly considered?

A

-derived from living things
-impossible to synthesize

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3
Q

produced urea

A

Friedrich Wohler

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4
Q

a compound excreted by mammals

A

Urea

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5
Q

What is urea made of?

A

by heating ammonium cyanate which is an inorganic mineral

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6
Q

What are the properties of organic compounds?

A
  1. All organic compounds contain carbon atoms and mostly contain hydrogen atoms.
  2. Carbon forms single, double, and triple bonds to carbon atom.
  3. Some compounds have chains of atoms and some compounds have rings.
  4. Organic compounds may also contain other than carbon and hydrogen.
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7
Q

any atom that is not carbon or hydrogen is called?

A

Heteroatom

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8
Q

What are the most common heteroatoms?

A

nitrogen, oxygen, halogens (f, cl, br, and i)

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9
Q

is an atom or a grp of atoms with a characteristic chemical and physical properties

A

Functional Groups

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10
Q

What are the Functional Grp contains?

A

a heteroatom, a multiple bond, or sometimes both

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11
Q

3 Types of Functional Grp

A

-hydrocarbons
-compounds with a single bond to a heteroatom
-compounds with a carbonyl grp

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12
Q

contains C and H only

A

Hydrocarbons

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13
Q

Most of the mass is in _____?

A

Nucleus

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14
Q

Most of the volume is in ______?

A

Electron Cloud

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15
Q

dense nucleus containing protons and neutrons, surrounded by an electron cloud containing electrons in a large vol. of space

A

Atomic Structure

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16
Q

same no. of protons but different no. of neutrons

A

Isotopes

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17
Q

the exact location of the electron cannot be known

A

Quantum Mechanical Model

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18
Q

the probability that the electron will be in a certain region of space at a given instant

A

Electron Density

19
Q

used to describe orbitals

A

Quantum Numbers

20
Q

describes the orbitals occupied by the atom’s electrons when they are all in the available orbitals with the lowest energy

A

Ground-state electron configuration

21
Q

What is Core and Valence electrons?

A

Core is the electrons below the outermost shell and Valence is electrons in the outermost shell

22
Q

an attractive force between two ions or between two atoms

A

Chemical Bond

23
Q

Why do chemical bonds form?

A

because the compound that results is more stable and lower in energy that the separate atoms

24
Q

an atom is most stable if it’s outer shell is either filled or contains eight electrons, and it has no electrons of higher energy

A

Octet Rule

25
Q

How do chemical bonds form?

A

Octet rule

26
Q

attractive forces between opposite charges

A

Electrostatic attraction

27
Q

bond form as a result of the electrostatic attraction between ions of opposite charge

A

Ionic Bond

28
Q

bond formed as a result of sharing electrons between two nuclei

A

Covalent Bond

29
Q

compounds formed by covalent bonds

A

Molecular Compounds

30
Q

measure of the ability of an atom to pull the bonding electrons towards itself

A

Electronegativity

31
Q

What is nonpolar and polar covalent bond?

A

Nonpolar is with the same electronegativity while polar is with different electronegativity

32
Q

The electron-dot structure and line-bond structure

A

-Lewis structure
-Kekule structure

33
Q

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

A

Formal Charge

34
Q

omitting of the covalent bonds and listing atoms bonded to a particular carbon next to it

A

Condensed Structures

35
Q

carbon atoms aren’t usually shown

A

Skeletal Structures

36
Q

based on arrangement of atoms in a molecule

A

Molecular Geometry

37
Q

based on valence electron pairs around a central atom

A

Electron Pair Geometry

38
Q

a model for the prediction of molecular geometry based on the minimization of electron repulsion between regions of electron density around an atom

A

Valence-Shell Electron-Pair Repulsion (VSEPR) Model

39
Q

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

A

Valence Bond Theory

40
Q

assumes the formation of molecular orbitals from the atomic orbitals

A

Molecular Orbital Theory

41
Q

produces the molecular geometry of the molecule

A

Hybridization

42
Q

2 ways to combine atomic orbitals into molecular orbitals

A

Additive and Subtractive

43
Q

two individual line-bond structures

A

Resonance Forms

Orgchem (4 decks)

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