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Atoms bonds and groups > Deck 1 > Flashcards

Deck 1 Flashcards

1
Q

What are the main features of an atoms structure?

A
  • Protons+Neutrons make up the nucleus.
  • Nucleus is tiny compared with the total volume of an atom.
  • Nucleus is extremely dense and makes up almost all of the atoms mas.
  • Most of an atom consists of empty space between the tiny nucleus and and the electron shells.
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2
Q

What are the main features of an atoms structure?

A
  • Protons+Neutrons make up the nucleus.
  • Nucleus is tiny compared with the total volume of an atom.
  • Nucleus is extremely dense and makes up almost all of the atoms mas.
  • Most of an atom consists of empty space between the tiny nucleus and and the electron shells.
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3
Q

What are the main features of an atoms structure?

A
  • Protons+Neutrons make up the nucleus.
  • Nucleus is tiny compared with the total volume of an atom.
  • Nucleus is extremely dense and makes up almost all of the atoms mas.
  • Most of an atom consists of empty space between the tiny nucleus and and the electron shells.
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4
Q

What is the relative mass and charge of a proton?

A

Relative mass = 1

Relative charge = -1

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5
Q

What is the relative mass and charge of a neutron?

A

Relative mass= 1

Relative charge = 0

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6
Q

What is the relative mass and charge of an electron?

A

Relative mass = 1/2000

Relative charge = - 1

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7
Q

Isotopes of the same element have?

A
  • Different masses
  • The same number of protons and electrons
  • different numbers of neutrons in the nucleus.
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8
Q

What two numbers describe an element?

A

The atomic number(proton number)- the number of protons in the nucleus.
-The mass number(nucleon number) - the number of particles(protons and neutrons) in the nucleus.

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9
Q

How can you work out the number of neutrons an isotope has?

A

Subtract the mass number by the proton number.

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10
Q

For an isotope, relative isotopic mass=

A

atomic mass

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11
Q

When measuring atoms masses by comparing them to carbon-12, what assumptions have been made?

A
  • We have neglected the tiny contribution that electrons make to the mass of an atom.
  • We have taken the masses of both a proton and a neutron as 1.0u.
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12
Q

What does the weighted mean mass mean?

A

Most elements contain a mixture of isotopes, each in a different amount and with a different mass. We use the term “weighted mean mass” to account for the contribution made by each isotope to the overall mass of an element.

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13
Q

What does the contribution made by an isotope to the overall mass depend on?

A
  • the percentage abundance of the isotope

- the relative mass of the isotope

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14
Q

A sample of bromine contains 53% of bromine-79 and 47% of bromine-81. Determine the relative atomic mass of bromine.

A

79.94 ( Go to page 9 for an example )

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15
Q

What is the relative mass and charge of a proton?

A

Relative mass = 1

Relative charge = -1

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16
Q

What is the relative mass and charge of a neutron?

A

Relative mass= 1

Relative charge = 0

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17
Q

What is the relative mass and charge of an electron?

A

Relative mass = 1/2000

Relative charge = - 1

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18
Q

Isotopes of the same element have?

A
  • Different masses
  • The same number of protons and electrons
  • different numbers of neutrons in the nucleus.
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19
Q

What two numbers describe an element?

A

The atomic number(proton number)- the number of protons in the nucleus.
-The mass number(nucleon number) - the number of particles(protons and neutrons) in the nucleus.

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20
Q

How can you work out the number of neutrons an isotope has?

A

Subtract the mass number by the proton number.

21
Q

For an isotope, relative isotopic mass=

A

atomic mass

22
Q

When measuring atoms masses by comparing them to carbon-12, what assumptions have been made?

A
  • We have neglected the tiny contribution that electrons make to the mass of an atom.
  • We have taken the masses of both a proton and a neutron as 1.0u.
23
Q

What does the weighted mean mass mean?

A

Most elements contain a mixture of isotopes, each in a different amount and with a different mass. We use the term “weighted mean mass” to account for the contribution made by each isotope to the overall mass of an element.

24
Q

What does the contribution made by an isotope to the overall mass depend on?

A
  • the percentage abundance of the isotope

- the relative mass of the isotope

25
Q

A sample of bromine contains 53% of bromine-79 and 47% of bromine-81. Determine the relative atomic mass of bromine.

A

79.94 ( Go to page 9 for an example )

26
Q

What is the relative mass and charge of a proton?

A

Relative mass = 1

Relative charge = -1

27
Q

What is the relative mass and charge of a neutron?

A

Relative mass= 1

Relative charge = 0

28
Q

What is the relative mass and charge of an electron?

A

Relative mass = 1/2000

Relative charge = - 1

29
Q

Isotopes of the same element have?

A
  • Different masses
  • The same number of protons and electrons
  • different numbers of neutrons in the nucleus.
30
Q

What two numbers describe an element?

A

The atomic number(proton number)- the number of protons in the nucleus.
-The mass number(nucleon number) - the number of particles(protons and neutrons) in the nucleus.

31
Q

How can you work out the number of neutrons an isotope has?

A

Subtract the mass number by the proton number.

32
Q

For an isotope, relative isotopic mass=

A

atomic mass

33
Q

When measuring atoms masses by comparing them to carbon-12, what assumptions have been made?

A
  • We have neglected the tiny contribution that electrons make to the mass of an atom.
  • We have taken the masses of both a proton and a neutron as 1.0u.
34
Q

What does the weighted mean mass mean?

A

Most elements contain a mixture of isotopes, each in a different amount and with a different mass. We use the term “weighted mean mass” to account for the contribution made by each isotope to the overall mass of an element.

35
Q

What does the contribution made by an isotope to the overall mass depend on?

A
  • the percentage abundance of the isotope

- the relative mass of the isotope

36
Q

A sample of bromine contains 53% of bromine-79 and 47% of bromine-81. Determine the relative atomic mass of bromine.

A

79.94 ( Go to page 9 for an example )

37
Q

What is the equation relating amount if substance n, mass m and molar mass M?

A

n=m/M
n=amount of substance
m=mass, in g
M= molar mass, in g mol^-1

38
Q

Empirical formula

A

The empirical formula is the simplest whole-number ratio of atoms of each element present in a compound.

39
Q

Analysis showed that 0.6075 g of magnesium combines with 3.995 g of bromine to form a compound.

A

Empirical formula MgBr2

40
Q

Analysis of a compound showed the following percentage composition by mass:
Na: 74.10% , O:25.81%
Find the ratio of atoms.

A

Na2O

41
Q

What is the molecular formula used for?

A

It is used fro compounds that exist as simple molecules.

42
Q

What does a molecular formula tell you?

A

A molecular formula tells you the number of each type of atom that make up a molecule.

43
Q

A compound has an empirical formula of CH2 and a relative molecular formula mass, Mr, of 56.0. What is its molecular formula?

A

C4H8

44
Q

What is the equation relating the amount of has molecules,n, in mol , the gas volume, V, in dm^3.

A

n=V/24dm^3
( this is because all substances take up the same amount of volume as gases providing they have the same number of moles )

45
Q

What is the volume, in cm^3, of 2.130 x 10^-3 mol of a gas at RPT?

A

51.12cm^3

46
Q

What does a concentration of a solution tell you?

A

The concentration of a solution tells you how much solute is dissolved in the solvent.

47
Q

What does a solution of 2 mol dm^-3 tell you?

A

There are 2 moles of solute dissolved in every 1dm^3 of solution.

48
Q

What equation relates the amount of substance, concentration of solute and volume of solution?

A 
n = c x V
Where:
- n= amount of substance, in mol.
- c= concentration of solute, in mol dm^-3
- V= volume of solution, in dm^3
49
Q

What is the amount, in mol, of NaOH dissolved in 25.0cm^3 of an aqueous solution of concentration 0.0125mol dm^-3?

A

3.125 x 10^-4 mol

Atoms bonds and groups (13 decks)

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