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Chemistry 2025 > U1; Atomic Structure and Periodic Trends > Flashcards

U1; Atomic Structure and Periodic Trends Flashcards

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1
Q

Define electron cloud

A

Region of space where there is a probability of an electron being found

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2
Q

Define nucleus

A

Small, dense protons and neutrons

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3
Q

What is the relative charge of an electron?

A

1-

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4
Q

What is the relative charge of a proton?

A

1+

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5
Q

What is the relative charge of a neutron?

A

0

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6
Q

What is the relative mass of an electron?

A

1/1836

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7
Q

What is the relative mass of a proton?

A

1

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8
Q

What is the relative mass of a neutron?

A

1

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9
Q

Explain Bohr’s model in relation to the emmision spectra and excited/ground state?

A

As an element is heated, electrons absorb energy and can be ‘promoted’ to a higher energy state known as ‘excited state’. Shortly afterwards, the electron ‘relapses’ to the lower energy state known as ‘ground state’ releasing a fixed amount of energy (a photon) as electromagnetic radiation (eg light)

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10
Q

Explain energy levels and shells

A

Further away from nucleus means more energy. Increasing energy further away from nucleus.

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11
Q

Name the four subshells

A

s,p,d,f

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12
Q

What is subshell capacity of s ?

A

2

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13
Q

What is subshell capacity of p ?

A

6

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14
Q

What is subshell capacity of d ?

A

10

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15
Q

What is subshell capacity of f ?

A

14

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16
Q

How many orbitals in s subshell?

A

1

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17
Q

How many orbitals in p subshell?

A

3

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18
Q

How many orbitals in d subshell?

A

5

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19
Q

How many orbitals in f subshell?

A

7

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20
Q

Summarize the Aufbau Principle

A

Electrons move into subshells in order from lowest energy to highest energy

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21
Q

Summarize Pauli’s Exclusion Principle

A

A maximum of 2 electrons may occupy an orbital (provided they have opposite spin)

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22
Q

Summarize Hund’s Rule

A

All orbitals in a subshell will be half-filled before completely filled. (singles before doubles)

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23
Q

When writing electron configurations for transition metal atoms in period 4, what happens? And what does this tell us?

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A

They lose their 4s electrons before their 3d electrons. It tells us that a filled 4s shell is greater energy than a half - filled 3d subshell.

24
Q

What is the electron configuration of Al - 13 (3+)

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A

(1s2, 2s2, 2p6) ^3+

25
Acid + Base
Salt + water
26
Acid + Metal Oxide
Salt + water
27
Acid + Metal Hydroxide
Salt + water
28
Acid + Metal
Salt + hydrogen
29
Acid + Metal Carbonate
Salt + water + carbon dioxide
30
Summarize the difference between an atom in its ground state and an atom in its excited state
An atom in its ground state has all electrons in their lowest possible subshell (in respect to energy) WHEREAS An atom in an excited state temporarily has one or more electrons in a higher energy subshell than the lowest possible
31
What happens because of a relapse off an atom from excited to ground state?
Light is emitted.
32
Write the subshell electronic configuration of S - 16 ^2-
( 1s2, 2s2, 2p6, 3s2, 3p6 )^2-
33
What is the ACTUAL electron configuration for copper?
1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10
34
What is the ACTUAL electron configuration for chromium?
1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d5
35
What two factors affect atomic radius?
1. Number of occupied energy levels (shells) 2. Core charge
36
Define Core Charge
A measure of the net attractive force felt by valence shell electrons towards the nucleus.
37
What is the formula to calculate core charge?
Number of protons in nucleus (nuclear charge) - the number of electrons in the inner shells
38
What is the core charge of sodium?
11-10 = 1+
39
What is the trend in atomic radii down a group of the Periodic table? And the explanation why
As you move down a group, the atomic radii increase. B/C -The number of occupied energy levels increases -Core charge remains constants > if higher core charge, nucleus has stonger attraction to electrons = decreased atomic radii
40
Explain Atomic Radii
Half the distance between two nuclei of a diatomic molecule, assuming a single covalent bond between two identical atoms.
41
What is the trend in atomic radii across a period of the Periodic table? And the explanation why
As you move across a period, the atomic radius decreases. B/C -The number of occupied shells remains constant -Core charge increases >This means that the valence electrons are more strongly attracted to the nucleus therefore decreased atomic radii.
42
Define Electronegativity
It is the strength with which atoms of an element attract electrons when they are chemically combined with another element.
43
What does a higher electronegativity mean?
It means the atoms are more able to pull the electrons that are shared in covalent bond towards their nucleus.
44
What do you need to mention in an electronegativity question?
-Atomic radii -Core charge -Occupied electron shells
45
What is the trend in electronegativity down a group of the periodic table?
As you move down a group the electronegativity decreases. B/C -number of occupied energy levels decreases t/f atomic radius increases -nuclear charge increases however due to electron shielding, core charge is same > t/f because their is less attraction of valence electrons towards nucleus, electronegativity decreases
46
What is the trend in electronegativity across a period of the periodic table?
As you move across a period, the electronegativity increases. B/C - number of occupied energy levels stays constant so atomic radius decreases (due to increasing core charge) -nuclear charge increases but number of shells stays same so core charge increases >t/f valence electrons are more attracted to nucleus thus increasing electronegativiy
47
What does electron shielding mean?
Number of inner shell electrons
48
Define the first ionization energy
The amount of energy required to remove an electron from each of a mole of gaseous atoms.
49
Write a half equation to describe first ionization of sodium
Na(g) > Na^+ (g) + e^-
50
What happens if we provide enough energy to excite an electron enough to move beyond all the possible electron shells?
The electron would escape the atom entirely - the atom will have been ionised.
51
What is the trend in ionization energy as you move down an group of the periodic table?
it will decrease because number of energy levels increases so atomic radii increases so less attraction to nucleus and core charge is constant so less energy required to remove an electron
52
What is the trend in ionization energy as you move across a period of the periodic table?
it will increase because atomic radii is decreasing so stronger attraction therefore more energy is required to lose an electron
53
Why is successive ionization energy harder?
Because removing negatively charged electron from a positive cation
54
What is the trend of reactivity of metal across a period?
decreases because they need to lose electrons to become a cation but hard to do so because of high first ionisation energy
55
What is the trend of reactivity of metals down a group?
it will increase down a group because easy to lose electrons
56
What is the trend of reactivity of non-metals down a group?
decreases
57
What is the trend of reactivity of metal across a period?
increases

Chemistry 2025 (6 decks)

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