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Chemistry > Unit 2 - BPA > Flashcards

Unit 2 - BPA Flashcards

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1
Q

Orbital definition

A

A region in an atom that can hold up to two electrons with opposite spin

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2
Q

Principle quantum number

A

Shell number

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3
Q

Electron shell definition

A

Group of atomic orbitals with the same principle quantum number

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4
Q

s-orbital shape

A

sphere

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5
Q

p-orbital shape

A

dumbell

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6
Q

Are 4s or 3d electrons removed first

A

4s

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7
Q

What type of forces hold the particles together in ionic bonding?

A

Electrostatic forces of attraction

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8
Q

What type of elements is ionic bonding between?

A

Non-metals and Metals

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9
Q

What type of elements is covalent bonding between?

A

Metals

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10
Q

Covalent bonding definition

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms

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11
Q

How many covalent bonds does Hydrogen make?

A

1

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12
Q

How many covalent bonds does Carbon make?

A

4

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13
Q

How many covalent bonds does Nitrogen make?

A

3

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14
Q

How many covalent bonds does Oxygen make?

A

2

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15
Q

Lone pair definiton

A

An unpaired pair of electrons

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16
Q

Bond enthalpy definition

A

The energy required to break a particular covalent bond in one molecule of a gaseous molecule

17
Q

Larger bond enthalpy

A

Stronger bond

18
Q

Linear bond angle

A

180

19
Q

Trigonal planar bond angle

A

120

20
Q

Tetrahedral bond angle

A

109.5

21
Q

Octahedral bond angle

A

90

22
Q

Electronegativity definition

A

The measure of an atoms ability to attract a pair of electrons towards itself

23
Q

Does electronegativity increase or decrease from left to right and down to up?

A

Increase

24
Q

Ionic bonding definition

A

Electrostatic attraction between positive and negative ions

25
Q

Order of intermolecular forces

A

Induced dipole-dipole interactions < Permanent dipole-dipole interactions < Hydrogen bonding

26
Q

Why is ice less dense than liquid water?

A

Hydrogen bonds are longer than Covalent bonds, causing an open lattice structure to form

27
Q

Why does water have a higher melting and boiling point than expected?

A

Hydrogen bonds are stronger than other intermolecular forces

28
Q

Hydrogen bond defininiton

A

A strong dipole-dipole interaction between an electron deficient hydrogen atom on one molecule and a lone pair of electrons on a very electronegative atom on a different molecule

Chemistry (3 decks)

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