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Chem 30A > Ch 1: Covalent Bonding and Shapes of Molecules > Flashcards

Ch 1: Covalent Bonding and Shapes of Molecules Flashcards

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1
Q

What do shells define?

A

The probability of finding an electron in a certain region

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2
Q

What is a shell?

A

A region of space surrounding the nucleus that can be occupied by electrons

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3
Q

What are 3 effects of shells?

A

Electrostatic attraction between the electrons and the nucleus, electrostatic repulsion between electrons, and the wavelike nature of an electron

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4
Q

What does it mean if something is quantized?

A

It has specific values rather than a continuum of values

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5
Q

What is delocalization?

A

The spreading of electron density over a larger volume of space

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6
Q

How many electrons can a shell hold?

A

2n² electrons, where n is the number of the shell

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7
Q

Electrons in the first shell are the _____ in energy.

A

lowest

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8
Q

Electrons in the higher-numbered shells are held _____.

A

less strongly than the electrons in the lower-numbered shells

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9
Q

Shells are divided into subshells given by _____ and within these subshells, electrons are grouped into _____.

A

s, p, d, f; orbitals

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10
Q

What is an orbital?

A

A region of space that can hold 2 electrons

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11
Q

What is the ground-state electron configuration of an atom or molecule?

A

the lowest electron configuration

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12
Q

What 3 rules determine ground-state electron configuration?

A

Aufbau Principle, Pauli Exclusion Principle, Hund’s Rule

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13
Q

What is the Aufbau Principle?

A

Orbitals are filled in order of increasing energy

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14
Q

What is the Pauli Exclusion Principle?

A

No more than 2 electrons can occupy an orbital, and they must have opposite (paired) spins

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15
Q

What is Hund’s Rule?

A

When degenerate orbitals are available, but there are not enough electrons to fill all of them completely, one electron is put in each before a second one is added to any.

The spins of the electrons in the degenerate orbitals should be parallel to reduce static repulsion- the convention is to have the spins going up.

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16
Q

What is energy?

A

the ability to do work

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17
Q

What is potential energy?

A

stored energy that is released when the object is released

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18
Q

What is an excited state?

A

a state of a system at a higher energy than the ground state

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19
Q

All of nature seeks _____.

A

its lowest energy state

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20
Q

When the electrons of an excited state are rearranged back to the ground state, _____.

A

the potential energy held by that unstable system is released and work is done

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21
Q

What is ionization potential?

A

the energy needed to remove an electron from an atom or molecule

22
Q

Electrons closest to the nucleus have the _____ionization potential , while electrons far from the nucleus have the _______ionization potential.

A

highest; lowest

23
Q

What is the octet rule?

A

Group 1A-7A elements react to achieve an outer shell of 8 valence electrons

24
Q

What is electronegativity?

A

a measure of an atom’s attraction for electrons

25
Q

What is electron affinity?

A

energy added or released when an electron is added to an atom or molecule

26
Q

Electronegativity _____ from top to bottom because _____.

A

decreases; the increasing distance of the valence shell from the nucleus results in a lower attraction between the electrons and the nucleus

27
Q

Electronegativity _____ from left to right because _____.

A

increases; the increasing positive charge on the nucleus results in a greater attraction for the valence electrons.

The orbitals get lower in energy as you move from left to right and the atoms hold their electrons tighter; these atoms have a higher first ionization potential.

28
Q

How is an ionic bond formed?

A

electrons are transferred from an atom of lower electronegativity to an atom of higher electronegativity

29
Q

An anion is formed by _____ electrons and is _____ charged.

A

gaining; negatively

30
Q

A cation is formed by _____ electrons and is _____ charged.

A

losing; positively

31
Q

What is the electronegativity difference between 2 atoms in an ionic bond?

A

> 1.9

32
Q

How is a covalent bond formed?

A

electrons are shared between atoms to complete the atoms’ valence shell

33
Q

What is bond dissociation entropy/enthalpy?

A

the amount of energy needed to be absorbed in order to break the bond

34
Q

What is the electronegativity difference between 2 atoms in a non polar covalent bond?

A

<0.5

35
Q

What is the electronegativity difference between 2 atoms in a polar covalent bond?

A

0.5 to 1.9

36
Q

In a polar covalent bond, the more electronegative atom _____, and the less electronegative atom _____.

A

gains a greater fraction of the electrons and has a partial negative charge; has a smaller fraction of the electrons and has a partial positive charge

37
Q

What is a bond dipole moment?

A

a measure of polarity of a polar covalent bond; the product of the charge on either atom of a polar covalent bond times the distance between the nuclei

38
Q

What is formal charge?

A

the charge on an atom in a polyatomic ion or molecule

39
Q

How do you calculate formal charge?

A

formal charge = #ve in neutral, unbonded atom - (all unshared e + ½ shared e)

40
Q

Why are functional groups important?

A
  • allow us to divide organic compounds into classes
  • exhibit characteristic chemical reactions
  • serve as a basis for naming compounds
41
Q

What is an alcohol?

A

a compound containing an -OH (hydroxyl) group bonded to a tetrahedral carbon atom

42
Q

What is an amine?

A

a compound containing a nitrogen atom bonded to one, two, or three carbon atom(s) by single bonds

43
Q

What is the functional group of both aldehydes and ketones?

A

a C=O (carbonyl) group

44
Q

What is an aldehyde?

A

a compound containing a -CHO group

45
Q

What is a ketone?

A

a compound containing a carbonyl group bonded to 2 carbons

46
Q

What is a carboxylic acid?

A

Compound containing a -COOH (carboxyl) group

47
Q

What is an ester?

A

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

48
Q

amide

A

Derivative if carboxylic acid in which the -OH is replaced by an amine

49
Q

What is VSEPR?

A

A method for predicting bond angles based on the idea that electrons repel each other and stay as far apart as possible

50
Q

molecular dipole moment

A

Vector sum of individual bond dipoles

51
Q

What 2 things do we need to determine the polarity of a molecule?

A

1)whether the molecule has polar bonds and 2)what the arrangement of its atoms is in space

Chem 30A (10 decks)

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