Chapter 5: Electron Structure, ionic bonding, and covalent bonding

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30 Terms

1
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maximum number of electrons in the first four shells:

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2
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shells are also known as…

energy levels

3
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formula for working out the maximum number of electrons in a shell:

2n2

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what is an orbital?

a region around the nucleus that can hold up to 2 electrons, with opposite spins

5
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how many electrons can an orbital hold?

2

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what are the 4 different kinds of orbital?

s-,p-,d-,f-

7
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what shape is an s-orbital?

spherical

<p>spherical </p>
8
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what shape is a p-orbital?

dumbbell

<p>dumbbell </p>
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from n = 2, how many separate p-orbitals are there in each shell?

3

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each shell from n = 3 contains how many d orbitals?

5

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each shell from n = 4 contains how many f orbitals?

7

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draw a diagram to show was orbitals, electrons, subshells, and principal quantum numbers are:

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what are subshells?

orbitals of the same type are grouped together as subshells

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electrons in the same orbital must have…

opposite spins → helps to counteract the repulsion between the negative charges of the 2 electrons.

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how do electrons fill up orbitals in sub shells?

  • by having one in each orbital before putting them in the same orbital

  • (bus analogy)

<ul><li><p>by having one in each orbital <strong><em>before </em></strong>putting them in the same orbital </p></li><li><p>(bus analogy) </p></li></ul><p></p>
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which is the higher energy level? 3d or 4s??

3d !! 4s fills up before → when written out, it is fine to put 3d before it though.

17
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shorthand electron configuration:

  • [previous noble gas in square brackets] continued notation

<ul><li><p>[previous noble gas in square brackets] continued notation </p></li></ul><p></p>
18
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with the 4s and 3d sub-shells, it is a case of…

first in, first out:

  • the 4s electrons are first in

  • the 4s electrons are first out

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an ionised element will have the same electron configuration as…

a different element

<p>a different element </p>
20
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def. ionic bonding:

the electrostatic attraction between positive and negative ions

21
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draw the ionic bonding for KF

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22
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what is a giant lattice structure??

a huge structure, where the atoms are innumerable:

  • each ion is surrounded by oppositely charged ions, forming a giant ionic lattice

23
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ionic compounds solubility:

  • dissolve in polar solvents

  • water molecules attract + surround ions

  • ionic lattice is broken down

compounds with large charges may not break down → attraction too strong in lattice

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why can’t ionic compounds conduct electricity in solid states?

  • ions are fixed in a position in the giant ionic lattice

  • there are no mobile charge carriers

<ul><li><p>ions are fixed in a position in the giant ionic lattice </p></li><li><p>there are no mobile charge carriers </p></li></ul><p></p>
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why are ionic compounds able to conduct electricity in liquid/dissolved in water?

  • solid ionic lattice breaks down

  • the ions are now free to move as mobile charge carriers

<ul><li><p>solid ionic lattice breaks down</p></li><li><p>the ions are now free to move as mobile charge carriers </p></li></ul><p></p>
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covalent bond def.

the overlap of atomic orbitals, each containing one electron, to give a shared pair of electrons.

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what is a lone pair:

a pair of electrons that are not in a covalent bond

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how many covalent bonds do carbon, nitrogen, oxygen, and hydrogen form?

  • carbon forms 4 bonds

  • nitrogen forms 3 bonds

  • oxygen forms 2 bonds

  • hydrogen forms 1 bond

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what is the expansion of the octet?

available from the n = 3 shell, there can be more than 8 electrons in the outer shell:

<p>available from the n = 3 shell, there can be more than 8 electrons in the outer shell: </p>
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what is a dative covalent bond?

  • originally a lone pair

  • both electrons are supplied by the same atom

<ul><li><p>originally a lone pair </p></li><li><p>both electrons are supplied by the same atom</p></li></ul><p></p>