Atomic Structure Flashcards

1
Q

What is the structure of an atom?

A
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2
Q

What is the relative mass and charge of protons?

A
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3
Q

What is the relative mass and charge of neutrons?

A
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4
Q

What is the relative mass and charge of electrons?

A
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5
Q

What is the mass number?

A
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6
Q

What is the atomic number?

A
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7
Q

Why do atoms have an overall neutral charge?

A
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8
Q

Why do atoms of the same element have the same chemical properties?

A
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9
Q

What are ions?

A
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10
Q

What are isotopes?

A
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11
Q

Why do isotopes of the same element have the same chemical properties but different physical properties?

A
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12
Q

What is relative atomic mass?

A

The average mass of an atom of an element compared to 1/12th of the mass of an atom of carbon-12.

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13
Q

What is relative isotopic mass?

A

The average mass of an atom of an isotope compared to 1/12th of the mass of an atom of carbon-12.

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14
Q

What is the equation to calculate the relative atomic mass?

A
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15
Q

What is the relative molecular mass ( Mr)?

A

The average mass of a molecule compared to 1/12th of the mass of an atom of carbon-12.

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16
Q

What does a mass spectometer do?

A

It shows you the relative atomic mass of an element or the relative abundance of its isotopes.

17
Q

What are the steps to mass spectroscopy?

A
  1. Ionisation.
  2. Acceleration.
  3. Ion drift.
  4. Detection.
18
Q

What happens during ionisation?

A
19
Q

What happens during acceleration?

A

The ions are accelerated by an electric field and the same amount of kinetic energy is applied to each ion. The lighter ions will accelerate more.

20
Q

What happens during ion drift?

A
21
Q

What happens during detection?

A
22
Q

How many orbitals and electrons does an s-subshell have?

A
23
Q

How many orbitals and electrons does an p-subshell have?

A
24
Q

How many orbitals and electrons does an d-subshell have?

A
25
Q

How many orbitals and electrons does an f-subshell have?

A
26
Q

What are the rules for figuring out the electronic configuration?

A
  1. Electrons fill up higher energy levels first.
  2. Electrons fill up orbitals singly first and then they pair up.
  3. An electron is removed from the highest energy level first.
27
Q

What is the different about the electronic configuration of transition metals like cooper and chromium?

A
  1. They only have one electron in the 4s subshell.
  2. When they become ions they lose electrons from their 4s subshell before their 3d subshell.
28
Q

What is the electronic configuration for chromium?

A
29
Q

What is the electronic configuration for cooper?

A
30
Q

What is the electronic configuration for Fe 2+?

A
31
Q

What is the first ionization energy?

A

The energy needed to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions.

32
Q

What factors affect ionisation energy?

A
  1. Nuclear charge.
  2. Distance from the nucleus.
  3. Shielding
33
Q

What is the second ionisation energy?

A
34
Q

Why are second ionisation energies higher compared to first ionisation energies?

A
35
Q

What is the trend in ionization energies as you go down group 2?

A
36
Q

What is the trend in ionization energies as you go across period 3?

A
37
Q

What are the exceptions to this rule in period 3?

A
38
Q

How can you use successive ionisation energies to figure out how many shells an atom has?

A