[Part 2]- C1- atomic structure ⚛️ Flashcards

1
Q

Fill in the gaps: Atoms are very small and have a radius of _ x __^-__ m

[Remember: this is about the current model of an atom!]

A
  • Fill in the gaps: Atoms are very small and have a radius of 1 x 10^-10m.
  • [also known as 0.1 nm]
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2
Q

Do atoms have an overall electrical charge? Explain your answer

A
  • No, atoms don’t have an overall electrical charge
  • This is because the number of electrons, is the same number of protons.
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3
Q
  • Fill in the gaps: The radius of a nucleus is less than 1/_, ___ of the radius of an atom.
  • Most of the atom is concentrated in the _______.
  • Hint: the current model of the atom
A
  • The radius of a nucleus is less than 1/10, 000 of the radius of an atom.
  • Most of the atom is concentrated in the nucleus.
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4
Q

[Easy] What is the relative mass and relative charge of a proton?

A

Relative mass: 1

Relative charge: +1

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5
Q

[Easy] What’s the relative mass and relative charge of a neutron?

Hint: charge is neutral

A

Relative mass: 1

Relative charge: 0

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6
Q

[Easy] What’s the relative mass and relative charge of an electron?

A

Relative mass: very small/0

Relative charge: -1

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7
Q

How do we work out the mass number of an element and the atomic number of an element?

A
  • Think M, for massive. Look for the biggest number in that individual element [of the periodic table]
  • atomic number [number of protons]- look at the smallest number
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8
Q

RECAP: What’s an isotope?

A

Isotopes are: atoms of the same element, with a different number of neutrons.

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9
Q

What’s an ion?

A
  • An ion is an atom, that has an overall charge. They have lost or gained electrons.
  • Positive ions= lost electrons
  • negative ions= gained electrons.
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10
Q

Fill in the gaps: In an atom, the number of electrons is equal to= the number of _______ in the nucleus.

A

In an atom, the number of electrons is equal to= the number protons in the nucleus.

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11
Q

What is the number of protons in an atom, of an element called?

A

Answer: atomic number.

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12
Q

What does the term ‘relative atomic mass’ mean?

A
  • relative atomic mass is always the biggest number on the periodic table (when we look at an element). We don’t have to calculate anything. Think m, for massive.
  • [the relative atomic mass, is the average of the mass numbers, of the different isotopes]
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13
Q

What’s the equation for calculating the relative atomic mass, based on mass number and percentage abundance [of an isotope] ?

Hint: not atom

A

Ar= (mass number of isotope 1 ✖️percent abundance of isotope 1) + (mass number of isotope 2 ✖️percentage abundance of isotope 2)
________________________________
100

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14
Q

How many electrons can the first energy level hold?

A
  • the first energy level can hold: 2 electrons
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15
Q

How many electrons can the second energy level hold?

A
  • the second energy level can hold: 8 electrons
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16
Q

How many electrons can the third energy level hold?

A
  • the third energy level can hold: 8 electrons
17
Q

How can many electrons can the fourth energy level hold?

Hint: ?> 12

A
  • the fourth energy level can hold 18 electrons