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Atomic Model And The Periodic Table Flashcards

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1
Q

What is matter?

A

Material, well defined samples of stuff.

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2
Q

Define mixtures.

A

Several substances mixed together.

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3
Q

What are substances?

A

Chemically pure samples containing one type of unit.

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4
Q

What is an element?

A

A substance containing atoms/nuclei of the same number of protons.

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5
Q

Define compounds.

A

A substance that contains atoms of two or more types combined in a fixed ratio.

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6
Q

What is an atom?

A

The basic building block of matter, made up of subatomic particles - protons, neutrons, and electrons.

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7
Q

What defines an element?

A

A substance composed of atoms with the same atomic number.

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8
Q

What is a compound?

A

A pure substance composed of atoms of two or more elements which have chemically combined in fixed proportions.

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9
Q

What is the mass number?

A

of protons + # of neutrons.

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10
Q

What is relative atomic mass?

A

The average mass of every type of one type of element/all different isotopes.

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11
Q

Fill in the blank: Matter can be broken down into ______, substances, elements, and compounds.

A

[mixtures]

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12
Q

True or False: Atoms can be broken down into the structure of neutrons, protons, and electrons.

A

True

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13
Q
A
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14
Q

What is the atomic number?

A

The number of protons in an atom

Atomic number determines the identity of an element.

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15
Q

Define isotopes.

A

Forms of the same element with different numbers of neutrons

Isotopes have the same atomic number but different mass numbers.

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16
Q

What is a cation?

A

A positively charged ion

Cations have more protons than electrons.

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17
Q

What is an anion?

A

A negatively charged ion

Anions have more electrons than protons.

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18
Q

Fill in the blank: Atomic mass = number of protons + _______.

A

number of neutrons

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19
Q

What is a polyatomic ion?

A

An ion made from a group of atoms

Examples include sulfate (SO4^2-) and ammonium (NH4^+).

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20
Q

True or False: Isotopes have the same atomic number but different mass numbers.

A

True

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21
Q

What effect do electrons and protons have on ions?

A

They determine whether the ion is a cation or an anion

Cations have more protons, while anions have more electrons.

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22
Q

What is the significance of the symbol of an element?

A

It represents the element in the periodic table

Each element has a unique symbol, such as Au for gold.

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23
Q

Fill in the blank: An ion is a group of atoms that are _______ charged.

A

positively or negatively

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24
Q

What does the term ‘relative atomic mass’ refer to?

A

The weighted average mass of an element’s isotopes

It is expressed in atomic mass units (amu).

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25
26
What did Niels Bohr propose in 1913 regarding electrons?
Electrons are arranged in shells (energy levels) around the nucleus
27
What does each shell correspond to in Bohr's model?
A specific level of energy
28
How is the amount of energy in each shell characterized?
It is unique for each element
29
What is the relationship between the shell's proximity to the nucleus and its energy?
The closer the shell is to the nucleus, the less energy it has
30
From which energy level shell are electrons filled first?
The lowest energy level shell
31
What are valence electrons?
Electrons in the outermost shell of an atom involved in chemical reactions
32
According to Rule 1, how many valence electrons can the outermost shell contain?
No more than 8 valence electrons
33
According to Rule 2, when will Shell 3 continue filling?
Only if there are at least two electrons in Shell 4 first
34
Fill in the blank: Electrons are arranged in ______ around the nucleus.
shells
35
True or False: The outermost shell can contain more than 8 valence electrons.
False
36
What is the significance of the outermost shell in terms of energy?
It requires the least energy to remove electrons
37
What happens to electrons in the outermost shell during chemical reactions?
They are involved in chemical reactions
38
39
What is the maximum number of electrons that the third shell can hold?
18 electrons ## Footnote The third shell can only accommodate 8 electrons until there are at least two in the fourth shell.
40
What happens to the electron configuration when an electron is excited?
Electrons jump to a higher energy level ## Footnote This results in a difference between ground and excited electron configurations.
41
How many electrons does Potassium have?
19 electrons ## Footnote The electron configuration for Potassium is 2, 8, 8, 1.
42
What is the electron configuration for Scandium?
2, 8, 11, 2 ## Footnote Scandium has 23 electrons.
43
Fill in the blank: The electron configuration of an atom ensures that all electrons are in the _______.
lowest possible energy levels ## Footnote This principle is essential for understanding electron arrangements.
44
What is the difference between ground state and excited state in electron configuration?
Valence electrons jump to a higher energy level ## Footnote This transition affects the atom's reactivity.
45
How many electrons are in the fourth shell when the third shell is filled?
2 electrons ## Footnote The third shell cannot contain more than 8 electrons until 2 electrons occupy the fourth shell.
46
What is the electron configuration of Vanadium?
2, 8, 11, 2 ## Footnote Vanadium has 23 electrons.
47
True or False: The third shell can be the outermost shell while having more than 8 electrons.
False ## Footnote The third shell cannot hold more than 8 electrons until the fourth shell has at least 2 electrons.
48
What is the maximum number of electrons that the third shell can hold?
18 electrons ## Footnote The third shell can only accommodate 8 electrons until there are at least two in the fourth shell.
49
What happens to the electron configuration when an electron is excited?
Electrons jump to a higher energy level ## Footnote This results in a difference between ground and excited electron configurations.
50
How many electrons does Potassium have?
19 electrons ## Footnote The electron configuration for Potassium is 2, 8, 8, 1.
51
What is the electron configuration for Scandium?
2, 8, 11, 2 ## Footnote Scandium has 23 electrons.
52
Fill in the blank: The electron configuration of an atom ensures that all electrons are in the _______.
lowest possible energy levels ## Footnote This principle is essential for understanding electron arrangements.
53
What is the difference between ground state and excited state in electron configuration?
Valence electrons jump to a higher energy level ## Footnote This transition affects the atom's reactivity.
54
How many electrons are in the fourth shell when the third shell is filled?
2 electrons ## Footnote The third shell cannot contain more than 8 electrons until 2 electrons occupy the fourth shell.
55
What is the electron configuration of Vanadium?
2, 8, 11, 2 ## Footnote Vanadium has 23 electrons.
56
True or False: The third shell can be the outermost shell while having more than 8 electrons.
False ## Footnote The third shell cannot hold more than 8 electrons until the fourth shell has at least 2 electrons.
57
58
What can a shell be further divided into?
Subshells ## Footnote Subshells are smaller levels within a shell.
59
How many types of subshells are there?
Four types of subshells: S, P, D, F ## Footnote Each type has different energy levels and electron configurations.
60
What is the relationship between shells and subshells?
Shell 1 has 1 subshell, Shell 2 has 2 subshells, Shell 3 has 3 subshells, Shell 4 and onwards has 4 subshells ## Footnote This hierarchy shows how subshells are organized within shells.
61
What are regions within subshells where electrons can be found called?
Orbitals ## Footnote Orbitals can hold up to 2 electrons each.
62
How many electrons can occupy an orbital?
Up to 2 electrons ## Footnote This is a fundamental rule in electron configurations.
63
What is the configuration of the subshells in Shell 1?
1s ## Footnote Shell 1 has only one subshell: 1s.
64
What is the configuration of the subshells in Shell 2?
2s, 2p ## Footnote Shell 2 consists of two subshells: 2s and 2p.
65
What is the configuration of the subshells in Shell 3?
3s, 3p, 3d ## Footnote Shell 3 includes three subshells: 3s, 3p, and 3d.
66
What is the configuration of the subshells in Shell 4?
4s, 4p, 4d, 4f ## Footnote Shell 4 and onwards have four subshells.
67
Fill in the blank: The energy levels of the subshells are ordered by the amount of _______.
protons ## Footnote The number of protons influences the electron configuration of an atom or ion.
68
True or False: Each subshell can only have one type of orbital.
False ## Footnote Each subshell can contain multiple orbitals of different types.
69
70
What is ionisation energy?
The minimum amount of energy required to remove an electron from an atom in gas form. ## Footnote Ionisation energy is a crucial concept in understanding how atoms interact and form ions.
71
What is the relationship between ionisation energy and valence electrons?
Ionisation energy is the minimum amount of energy required to remove a valence electron from an atom. ## Footnote Valence electrons are the outermost electrons involved in chemical bonding.
72
Provide an example of ionisation energy.
Na(g) → Na⁺(g) + e⁻ ## Footnote This equation represents the ionisation of sodium, where one electron is removed.
73
What is successive ionisation energy?
The minimum amount of energy required to remove another electron from an ion. ## Footnote Each successive ionisation energy is higher than the previous one due to increased nuclear attraction.
74
Give an example of successive ionisation energy.
Na⁺(g) → Na²⁺(g) + e⁻ ## Footnote This process shows the removal of a second electron from a sodium ion.
75
What happens to ionisation energy as more electrons are removed?
Successive ionisation energies increase. ## Footnote This is due to the decreased electron-electron repulsion and increased attraction of the remaining electrons to the nucleus.
76
Describe the trend in ionisation energy regarding electron shells.
Electrons in the first shell are more strongly attracted to the nucleus than those in higher shells. ## Footnote This results in lower ionisation energy for electrons in higher shells.
77
Fill in the blank: As more electrons are removed, the ionisation energy ______.
increases. ## Footnote This increase is due to the reduced shielding effect and increased effective nuclear charge.
78
True or False: The first ionisation energy is always the highest.
False. ## Footnote The first ionisation energy is usually lower than subsequent ionisation energies.
79
What is the effect of removing an electron from a shell on energy requirements?
It increases the energy required to remove additional electrons. ## Footnote Removing electrons from shells closer to the nucleus requires more energy due to stronger attraction.
80

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