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SESSION 1: Introduction to Chemistry Code: BIOB111 > Concept 1,2,3,4,5,6 > Flashcards

Concept 1,2,3,4,5,6 Flashcards

Concept 2: Arrangement of subatomic particles within an atom Concept 3: Atoms are neutral Concept 4: Atomic number Concept 5: Mass number Concept 6: Isotopes

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1
Q

The word atom is an ancient Greek word
that means

A
  1. undivided
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2
Q

Atoms contain subatomic particles, called?

A
  1. protons
  2. neutrons
  3. electrons
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3
Q

Dalton’s atomic theory

A
  1. • All matter is made up of tiny particles called atoms
  2. • Atoms are in constant motion
  3. • All atoms of the same element are identical
  4. • Atoms of any one element are different from those of any other element
  5. • Atoms are never created nor destroyed during a chemical reaction, only rearranged
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4
Q

Matter is made up of?

A
  1. Atoms
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5
Q

Atoms contain three different types of?

A
  1. Subatomic particles
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6
Q

What are the three difference subatomic particles?

A
  1. Electron
  2. Proton
  3. Neutron
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7
Q

Define a proton

A
  1. Positively charged subatomic particle in the nucleus
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8
Q

Define a Neutron

A
  1. Subatomic particle in the nucleus with a neutral charge
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9
Q

Define an electron

A
  1. Negatively charged subatomic particle, around the outside of the nucleus
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10
Q

Proton; charge, atomic mass unit and location

A
  1. Has 1 positive charge (P+)
  2. 1 atomic mass unit
  3. Located inside the nucleus with the neutrons
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11
Q

Neutron; charge, atomic mass unit and location

A
  1. Has NO charge, is neutral, does not repel or attract
  2. 1 atomic mass unit
  3. Located inside the nucleus with the proton
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12
Q

Electron; charge,atomic mass unit and location

A
  1. Has 1 negative charge (e-)
  2. electron mass is so small, it doesn’t count towards the atom mass
  3. Located outside the nucleus, in the electron cloud
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13
Q

What is amu?

A
  1. Atomic mass unit
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14
Q

describe the nucleus?

A
  1. nucleus is at the centre of the atom
  2. Protons & neutrons are tightly packed together in the nucleus.
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15
Q

Define electrons in relation to their locations and charge

A
  1. Orbit outside of the nucleus
  2. the negative charge of electrons is attracted to the positive charges of the protons in the nucleus
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16
Q

What is an electron shell?

A
  1. Electron shells contain a group of electrons with similar energies
  2. Electron shells are positioned a certain distance away from the nucleus
  3. Shell 1,2,3
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17
Q

Define electron shell 1

A
  1. Shell closest to the nucleus
  2. First shell that is filled with electrons
  3. Contains a maximum of 2 electrons
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18
Q

Define electron shell 2

A
  1. Shell 2nd closest to the nucleus
  2. Filled with electrons after shell 1 is full of
  3. Contains maximum 8 electrons
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19
Q

Define electron shell 3

A
  1. Shell 3rd closest to the nucleus
  2. Filled with electrons after shell 2 is full of electrons
  3. Contains a maximum of 18 electrons
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20
Q

The maximum number of electrons that can be placed into a shell?

A
  1. 2n2
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21
Q

Where are the electrons with the lowest energy located, and why?

A
  1. closest to the nucleus = electrons with the lowest energy
  2. these are highly attracted to the protons
  3. these need a low amount of energy to hold their position close to the nucleus
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22
Q

Where are the electrons with the highest energy located and why?

A
  1. furthest to the nucleus = electrons with higher energy
  2. these have a low attraction to the protons
  3. these need a high amount of energy to hold their position further away from the nucleus
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23
Q

Define an orbital

A
  1. A position in an electron shell
  2. where a maximum of 2 electrons are held
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24
Q

How many orbitals in shell 1?

A
  1. 1 orbital
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25
Q

How many orbitals in shell 2?

A
  1. 4 orbitals
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26
Q

explain how the electron shell is filled

A
  1. Each orbital must have one electron before any of the orbitals can have two electrons
27
Q

Describe the atomic mass scale

A
  1. used to determine how much mass is in
    • atoms
    • compounds
    • molecules
28
Q

What is an atom’s atomic mass?

A
  • the mass of an atom’s nucleus
    1. protons + neutrons
29
Q

Atomic nunber?

A
  1. number of protons in the nucleus
30
Q

Why are atoms neutral?

A
  1. equal number of positively + negatively charged subatomic particles
    • equal # of protons and electrons
31
Q

What is the atomic number equal to?

A
  1. number of protons in the nucleus
32
Q

Describe isotopes

A
  1. variants of a chemical element
  2. same number of protons/atomic number
  3. different number of neutrons
33
Q

Reversed Cards

  1. undivided
A

The word atom is an ancient Greek word
that means

34
Q

Reversed Cards

  1. protons
  2. neutrons
  3. electrons
A

Atoms contain subatomic particles, called?

35
Q

Reversed Cards

  1. • All matter is made up of tiny particles called atoms
  2. • Atoms are in constant motion
  3. • All atoms of the same element are identical
  4. • Atoms of any one element are different from those of any other element
  5. • Atoms are never created nor destroyed during a chemical reaction, only rearranged
A

Dalton’s atomic theory

36
Q

Reversed Cards

  1. Atoms
A

Matter is made up of?

37
Q

Reversed Cards

  1. Subatomic particles
A

Atoms contain three different types of?

38
Q

Reversed Cards

  1. Electron
  2. Proton
  3. Neutron
A

What are the three difference subatomic particles?

39
Q

Reversed Cards

  1. Positively charged subatomic particle in the nucleus
A

Define a proton

40
Q

Reversed Cards

  1. Subatomic particle in the nucleus with a neutral charge
A

Define a Neutron

41
Q

Reversed Cards

  1. Negatively charged subatomic particle, around the outside of the nucleus
A

Define an electron

42
Q

Reversed Cards

  1. Has 1 positive charge (P+)
  2. 1 atomic mass unit
  3. Located inside the nucleus with the neutrons
A

Proton; charge, atomic mass unit and location

43
Q

Reversed Cards

  1. Has NO charge, is neutral, does not repel or attract
  2. 1 atomic mass unit
  3. Located inside the nucleus with the proton
A

Neutron; charge, atomic mass unit and location

44
Q

Reversed Cards

  1. Has 1 negative charge (e-)
  2. electron mass is so small, it doesn’t count towards the atom mass
  3. Located outside the nucleus, in the electron cloud
A

Electron; charge,atomic mass unit and location

45
Q

Reversed Cards

  1. Atomic mass unit
A

What is amu?

46
Q

Reversed Cards

  1. nucleus is at the centre of the atom
  2. Protons & neutrons are tightly packed together in the nucleus.
A

describe the nucleus?

47
Q

Reversed Cards

  1. Orbit outside of the nucleus
  2. the negative charge of electrons is attracted to the positive charges of the protons in the nucleus
A

Define electrons in relation to their locations and charge

48
Q

Reversed Cards

  1. Electron shells contain a group of electrons with similar energies
  2. Electron shells are positioned a certain distance away from the nucleus
  3. Shell 1,2,3
A

What is an electron shell?

49
Q

Reversed Cards

  1. Shell closest to the nucleus
  2. First shell that is filled with electrons
  3. Contains a maximum of 2 electrons
A

Define electron shell 1

50
Q

Reversed Cards

  1. Shell 2nd closest to the nucleus
  2. Filled with electrons after shell 1 is full of
  3. Contains maximum 8 electrons
A

Define electron shell 2

51
Q

Reversed Cards

  1. Shell 3rd closest to the nucleus
  2. Filled with electrons after shell 2 is full of electrons
  3. Contains a maximum of 18 electrons
A

Define electron shell 3

52
Q

Reversed Cards

  1. 2n2
A

The maximum number of electrons that can be placed into a shell?

53
Q

Reversed Cards

  1. closest to the nucleus = electrons with the lowest energy
  2. these are highly attracted to the protons
  3. these need a low amount of energy to hold their position close to the nucleus
A

Where are the electrons with the lowest energy located, and why?

54
Q

Reversed Cards

  1. furthest to the nucleus = electrons with higher energy
  2. these have a low attraction to the protons
  3. these need a high amount of energy to hold their position further away from the nucleus
A

Where are the electrons with the highest energy located and why?

55
Q

Reversed Cards

  1. A position in an electron shell
  2. where a maximum of 2 electrons are held
A

Define an orbital

56
Q

Reversed Cards

  1. 1 orbital
A

How many orbitals in shell 1?

57
Q

Reversed Cards

  1. 4 orbitals
A

How many orbitals in shell 2?

58
Q

Reversed Cards

  1. Each orbital must have one electron before any of the orbitals can have two electrons
A

explain how the electron shell is filled

59
Q

Reversed Cards

  1. used to determine how much mass is in
    • atoms
    • compounds
    • molecules
A

Describe the atomic mass scale

60
Q

Reversed Cards

  • the mass of an atom’s nucleus
    1. protons + neutrons
A

What is an atom’s atomic mass?

61
Q

Reversed Cards

  1. number of protons in the nucleus
A

Atomic nunber?

62
Q

Reversed Cards

  1. equal number of positively + negatively charged subatomic particles
    • equal # of protons and electrons
A

Why are atoms neutral?

63
Q

Reversed Cards

  1. number of protons in the nucleus
A

What is the atomic number equal to?

64
Q

Reversed Cards

  1. variants of a chemical element
  2. same number of protons/atomic number
  3. different number of neutrons
A

Describe isotopes

SESSION 1: Introduction to Chemistry Code: BIOB111 (3 decks)

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