Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Organic Chemistry 1 > Introduction > Flashcards

Introduction Flashcards

(49 cards)

Start Studying
1
Q

What does the term ‘organic’ refer to in the context of chemistry?

A

Compounds based on carbon structures

Historically, it referred to compounds from living sources.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Who demonstrated that an organic compound could be synthesized from a mineral source?

A

Wöhler in 1828

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are organic compounds typically used in?

A

Biological molecules, drugs, solvents, dyes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What does the atomic number (Z) represent?

A

The number of protons in the atom’s nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the mass number (A)?

A

The number of protons plus neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Define isotopes.

A

Atoms of the same element with different numbers of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the atomic mass of an element?

A

The weighted average mass of an element’s naturally occurring isotopes in atomic mass units (amu)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is a wave function in quantum mechanics?

A

A solution of the wave equation describing electron energies and locations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are the four types of atomic orbitals?

A

s, p, d, f

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does the first shell of an atom contain?

A

One s orbital (1s) that holds two electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How many p orbitals are present in each shell?

A

Three perpendicular p orbitals: px, py, and pz

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the Aufbau principle?

A

Lowest-energy orbitals fill first

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What does the Pauli exclusion principle state?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is Hund’s rule?

A

Electrons occupy degenerate orbitals singly with parallel spins before pairing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the significance of carbon’s four bonds in chemical bonding theory?

A

It allows carbon to form stable compounds by sharing electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is a covalent bond?

A

A bond formed by the sharing of electrons between atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How many valence electrons does carbon have?

A

Four valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are nonbonding electrons?

A

Valence electrons that are not used in bonding, also known as lone-pair electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is hybridization in chemistry?

A

The mixing of atomic orbitals to form new hybrid orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the bond angle in a tetrahedral structure?

21
Q

What type of bond is formed between two sp3 hybridized carbon atoms in ethane?

Study These Flashcards
A

Sigma (σ) bond

22
Q

What is the bond length of a C-C bond in ethane?

23
Q

What is the bond angle in ethylene?

24
Q

What is a π bond?

Study These Flashcards
A

A bond formed by the side-to-side overlap of p orbitals

25
What is the bond length of the C=C bond in ethylene?
133 pm
26
What type of hybridization occurs in acetylene?
sp hybridization
27
What is the bond angle in sp hybridized molecules?
180°
28
What is the molecular orbital theory?
A theory that describes the behavior of electrons in molecules using molecular orbitals
29
What is the difference between bonding and antibonding molecular orbitals?
Bonding MOs are lower in energy, while antibonding MOs are higher in energy
30
What is the chemistry of carbon compounds known as?
Organic chemistry ## Footnote Organic chemistry focuses on the structure, properties, composition, reactions, and synthesis of carbon-containing compounds.
31
What is the structure of an atom?
Positively charged nucleus surrounded by negatively charged electrons ## Footnote The nucleus contains protons and neutrons, while electrons are found in orbitals around the nucleus.
32
How is the electronic structure of an atom described?
By wave equation ## Footnote The wave equation helps in understanding the behavior of electrons in an atom.
33
What do electrons occupy around the nucleus?
Orbitals ## Footnote Orbitals are regions in an atom where there is a high probability of finding electrons.
34
What shape do s orbitals have?
Spherical ## Footnote S orbitals are spherical in shape and have no angular nodes.
35
What shape do p orbitals have?
Dumbbell-shaped ## Footnote P orbitals consist of two lobes and have one angular node.
36
What is a covalent bond?
An electron pair shared between atoms ## Footnote Covalent bonds are formed when two atoms share one or more pairs of electrons.
37
What theory describes electron sharing by overlap of atomic orbitals?
Valence bond theory ## Footnote Valence bond theory explains how atomic orbitals combine to form covalent bonds.
38
What does molecular orbital (MO) theory state?
Bonds result from combination of atomic orbitals to give molecular orbitals ## Footnote Molecular orbitals are delocalized over the entire molecule and can be bonding or antibonding.
39
What is the shape and formation method of sigma (σ) bonds?
Circular cross-section formed by head-on interaction ## Footnote Sigma bonds are the strongest type of covalent bond and allow for free rotation around the bond axis.
40
What is the shape of pi (π) bonds and how are they formed?
Dumbbell shape from sideways interaction of p orbitals ## Footnote Pi bonds are generally weaker than sigma bonds and do not allow for rotation.
41
What type of hybrid orbitals does carbon use in single bonds with tetrahedral geometry?
sp3 hybrid orbitals ## Footnote The sp3 hybridization involves the mixing of one s orbital and three p orbitals.
42
What hybridization does carbon use in double bonds with planar geometry?
sp2 hybrid orbitals and one unhybridized p orbital ## Footnote In sp2 hybridization, one s orbital and two p orbitals mix, while one p orbital remains unhybridized.
43
What hybridization does carbon use to form a triple bond with linear geometry?
sp hybrid orbitals and two unhybridized p orbitals ## Footnote The sp hybridization involves one s orbital and one p orbital, with two p orbitals remaining unhybridized.
44
What atoms hybridize to form strong, oriented bonds?
Nitrogen and oxygen ## Footnote Hybridization in these atoms allows them to form stable covalent bonds with specific geometries.
45
What type of hybridization does the nitrogen atom in ammonia exhibit?
sp3 hybridized ## Footnote This results in a trigonal pyramidal geometry for ammonia.
46
What type of hybridization does the oxygen atom in water exhibit?
sp3 hybridized ## Footnote This hybridization leads to a bent molecular geometry for water.
47
Fill in the blank: The π bonding MO is formed from combining _______ with the same algebraic sign.
p orbital lobes ## Footnote The combination leads to a lower energy state for the molecule.
48
Fill in the blank: The π antibonding MO is formed from combining lobes with _______.
opposite signs ## Footnote This combination results in a higher energy state for the molecule.
49
True or False: Only the bonding MO is occupied in ethylene.
True ## Footnote The antibonding MO remains unoccupied in stable molecules.

Organic Chemistry 1 (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions