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Gen, Org, and Inorg Chemistry > Introduction to organic chemistry > Flashcards

Introduction to organic chemistry Flashcards

1
Q

Organic compounds are made up of _________ and only a few other elements.

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

carbon

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2
Q

sulfur, phosphorus, and a halogen are present in some organic compounds. True or False

A

True

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3
Q

approximately 95% of all known compounds are organic. True or False

A

False - 85%

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4
Q

A belief that organic compounds can only be made with the aid of the mysterious vital force present only in living organic compounds.

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Vitalism

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5
Q

The German chemist that debunked vitalism and demonstrated the conversion of ammonium cyanate (a known inorganic salt) into urea.

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Friedrich Wöhler

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6
Q

inorganic compounds are just simply defined as compounds containing carbon atoms, while organic compounds are those compounds lacking carbon. True or False

A

False - organic compounds are just simply defined as compounds containing carbon atoms, while inorganic compounds are those compounds lacking carbon.

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7
Q

The compound formula is adequate to define because compounds differ in how atoms are bonded together. True or False

A

False - not adequate

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8
Q

compounds with the same molecular formula but different structures.

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Constitutional isomers

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9
Q

Carbon is a tetravalent element. True or False

A

True

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10
Q

Hydrogen and halogens is a monovalent element. True or False

A

True

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11
Q

Nitrogen and Oxygen are both trivalent elements. True or False

A

False - oxygen is a divalent element

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12
Q

Dimethyl ether and ethanol are samples of constitutional isomers. True or False

A

True

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13
Q

an atom or group of atoms within a molecule that shows a characteristic set of predictable physical and chemical properties.

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Functional group

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14
Q

Functional groups undergo the same types of chemical reactions no matter in what organic molecule they are found. True or False

A

True

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15
Q

Functional groups provide the basis on which

we derive names for organic compounds. True or False

A

True

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16
Q

Contain an -OH (hydroxyl) group bonded to a tetrahedral carbon atom.

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Alcohol

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17
Q

Ethanol and Methanol is alcohol. True or False

A

True

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18
Q

Primary alcohol contains 1 carbon group/2 hydrogen attached to COH. True or False

A

True

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19
Q

has 3 carbon groups/ 0 hydrogen attached to COH

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Tertiary

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20
Q

Secondary alcohols has 2 carbon groups/ 1 hydrogen attached to COH. True or False

A

True

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21
Q

a compound containing an amino group (-NH2, RNH2, R2NH, R3N).

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Amine

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22
Q

Secondary amine has a 2 Hydrogen attached to the nitrogen. True or False

A

False - Primary

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23
Q

Tertiary amine has 0 Hydrogen attached to the nitrogen. True or False

A

True

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24
Q

contains a carbonyl group (C=O) bonded to hydrogen.

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Aldehyde

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25
Q

The simplest aldehyde; the carbonyl group is bonded to two hydrogens.

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Formaldehyde

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26
Q

contains a carbonyl group (C=O) bonded to two carbon atoms.

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Ketone

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27
Q

a compound containing a -COOH (carboxyl: carbonyl + hydroxyl) group.

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Carboxylic acid

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28
Q

derivative of a carboxylic acid in which the H of the carboxyl group is replaced by a carbon group.

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Carboxylic ester

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29
Q

derivative of a carboxylic acid in which the -OH of the carboxyl group is replaced by an amino group.

CHOICES:
Alcohol, Amine, Formaldehyde, Ketone, Amide, Carboxylic ester, Carboxylic acid, Aldehyde, Tertiary

A

Amide

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30
Q

He defined a covalent bond as a result of two atoms sharing a pair of electrons

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Gilbert Lewis

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31
Q

between positively charged nuclei and negatively charged electrons

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Attractive forces

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32
Q

between two positively charged nuclei

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Repulsive forces

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33
Q

between two negatively charged electrons

CHOICES:
Attractive forces, Vitalism, carbon, Repulsive forces, Gilbert Lewis, Friedrich Wöhler, Functional group, Constitutional isomers

A

Repulsive forces

34
Q

electrons in the outermost shell.

CHOICES:
Nonpolar covalent bond, Polar covalent bond, Quantum Mechanics, Ionic bond, Electronegativity, Valence electrons

A

Valence electrons

35
Q

We can calculate the number of valence electrons by analyzing the electronic configuration. True or False

36
Q

how strongly an atom attracts shared electrons.

CHOICES:
Nonpolar covalent bond, Polar covalent bond, Quantum Mechanics, Ionic bond, Electronegativity, Valence electrons

A

Electronegativity

37
Q

electrons shared between two atoms, where electronegativity difference is less than 0.5.

CHOICES:
Nonpolar covalent bond, Polar covalent bond, Quantum Mechanics, Ionic bond, Electronegativity, Valence electrons

A

Nonpolar covalent bond

38
Q

electrons shared between two atoms with electronegativity difference between 0.5 and 1.7.

CHOICES:
Nonpolar covalent bond, Polar covalent bond, Quantum Mechanics, Ionic bond, Electronegativity, Valence electrons

A

Polar covalent bond

39
Q

the electrons are transferred producing ions; the two atoms have an electronegativity difference of more than 1.7, and so the more electronegative atom owns the electrons.

CHOICES:
Nonpolar covalent bond, Polar covalent bond, Quantum Mechanics, Ionic bond, Electronegativity, Valence electrons

A

Ionic bond

40
Q

established as a theory to explain the wave properties of electrons

CHOICES:
Nonpolar covalent bond, Polar covalent bond, Quantum Mechanics, Ionic bond, Electronegativity, Valence electrons

A

Quantum Mechanics

41
Q

The solution to wave equations are wave functions. The 3D plot of a (Ψ2) gives an image of an atomic orbital. True or False

42
Q

The placement of electrons is governed by the following: Aufbau principle, Pauli exclusion principle, and Hund’s Rule. True or False

43
Q

the overlapping of atomic orbital space between two or more atoms.

CHOICES:
Sigma (s) bond, Hybridization, pi bond, Antibonding molecular orbital, Molecular orbital

A

Sigma (s) bond

44
Q

overlapping atomic orbital wavefunctions that extend over the entire molecule

CHOICES:
Sigma (s) bond, Hybridization, pi bond, Antibonding molecular orbital, Molecular orbital, Valence shell electron pair repulsion (VSEPR) theory

A

Molecular orbital

45
Q

consists of destructive interference where no bonds are formed.

CHOICES:
Sigma (s) bond, Hybridization, pi bond, Antibonding molecular orbital, Molecular orbital, Valence shell electron pair repulsion (VSEPR) theory

A

Antibonding molecular orbital

46
Q

Antibonding molecular
bonds have lower energy
because it has one node. True or False

A

False - higher energy

47
Q

explains how carbon forms four bonds with equal atomic orbitals (tetravalent).

CHOICES:
Sigma (s) bond, Hybridization, pi bond, Antibonding molecular orbital, Molecular orbital, Valence shell electron pair repulsion (VSEPR) theory

A

Hybridization

48
Q

The ground-state electron configuration for carbon explains how carbon makes four bonds. True or False

A

False - it cannot explain

49
Q

considering the excited state, it still doesn’t explain how carbon makes 4 equivalent bonds, like the 4 to H in a methane molecule. True or False

50
Q

The p orbitals overlap to form a ___________. Pi bonds are weaker than sigma bonds.

CHOICES:
Sigma (s) bond, Hybridization, pi bond, Antibonding molecular orbital, Molecular orbital, Valence shell electron pair repulsion (VSEPR) theory

51
Q

Carbon naturally forms four bonds through hybridization which results to tetrahedral molecular geometry. True or False

52
Q

If C has 4 single bonds: sp4 hybridized. True or False

A

False - sp3

53
Q

If C has 1 double bond and

2 single bonds: sp2 hybridized. True or False

54
Q

If C has 1 triple bond and 1

single bond: no sp is hybridized. True or False

A

False - only sp is hybridized

55
Q

stronger than pi bond as it requires almost twice the bind energy of a pi bond to break it.

CHOICES:
Sigma (s) bond, Hybridization, pi bond, Antibonding molecular orbital, Molecular orbital, Valence shell electron pair repulsion (VSEPR) theory

A

Sigma bond

56
Q

Bond strength and bond length are inversely proportional. True or False

57
Q

More bonds =longer bond length. Hence, sp3>sp2>sp. True or False

A

False - shorter bond strength

58
Q

More bonds = higher bond strength. Hence, sp3

59
Q

valence electrons (shared and lone pairs) repel each other

CHOICES:
Sigma (s) bond, Hybridization, pi bond, Antibonding molecular orbital, Molecular orbital, Valence shell electron pair repulsion (VSEPR) theory

A

Valence shell electron pair repulsion (VSEPR) theory

60
Q

To identify its molecular geometry, determine its steric number. True or False

61
Q

For any sp3 hybridized atom, the 4 valence electron pairs will form a tetrahedral molecular geometry
with a 119.5° bond angle. True or False

A

False - 109.5°

62
Q

For any sp2 hybridized atom, the electron pairs will form a trigonal planar molecular geometry with a 140° bond angle. True or False

A

False - 120°

63
Q

For any sp hybridized atom, the electron pairs will form a linear molecular geometry with a 180° bond angle. True or False

64
Q

Electronegativity differences result in ___________

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

polar bonds

65
Q

___________ is the shifting electrons within an orbital results in a dipole moment.

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

66
Q

(the amount of partial charge) x (the distance the 8+ and 8- are separated)

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Dipole moment

67
Q

For molecules with multiple polar bonds, the dipole moment is the vector sum of all the individual bond dipoles. True or False

68
Q

often used to give a visual depiction of polarity

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Electrostatic potential maps

69
Q

____________ are attracted to one another through Dipole-dipole interactions, Hydrogen bonding, Dispersion forces

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Neutral molecules

70
Q

polar molecules line up their opposite charges.

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Dipole-dipole forces

71
Q

essentially strong type of dipole-dipole attraction because the partial + and – charges are relatively large.

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Hydrogen bonds

72
Q

solvents that engage in H-bonding.

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Protic solvents

73
Q

solvents that do not form H-bonds.

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Aprotic solvents

74
Q

Increasing the amount and extent of hydrogen bonding explains why the following isomers have different boiling points. True or False

75
Q

H-bonds are among the forces that cause DNA to form a double helix and some proteins to fold into an alpha-helix. True or False

76
Q

weakest IMF present between all molecules (polar or nonpolar).

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

London dispersion forces

77
Q

London dispersion forces are the reason why molecules with more mass generally have lower boiling points. True or False

A

False - higher

78
Q

The more branching in a molecule, the lower its surface area, and the weaker the London dispersion forces. True or False

79
Q

generally, it mixes well with
other polar compounds

CHOICES:
polar bonds, Dipole moment, Dipole-dipole forces, Hydrogen bonds, Polar compounds, London dispersion forces, Aprotic solvents, Protic solvents, Neutral molecules, Electrostatic potential maps, Induction

A

Polar compounds

80
Q

the principle of solubility is like-dissolves-like. True or False

Gen, Org, and Inorg Chemistry (15 decks)

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