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IBChemistryDPHLFlashcardsModels of the Particulate Nature of MatterThe Nuclear Atom

The Nuclear Atom (DP IB Chemistry)

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  • What is the mass and charge of a proton?

    A proton has a relative mass of 1 and a charge of +1.

  • What is the relative mass and charge of an electron?

    An electron has a negligible mass and a charge of -1.

  • Which subatomic particles are in the nucleus of an atom?

    The subatomic particles in the nucleus of an atom are protons and neutrons.

  • True or False?

    Atoms are made of subatomic particles.

    True.

    Atoms are made of subatomic particles including protons, neutrons, and electrons.

  • True or False?

    Electrons have a larger mass than protons.

    False.

    Electrons have a much smaller mass than protons.

  • Which sub-atomic particle is not found inside the nucleus?

    The sub-atomic particle that is not found inside the nucleus is the electron.

  • What is the relative mass and charge of a neutron?

    An neutron has a relative mass of 1 and charge of 0.

  • True or False?

    The nucleus of an atom has no charge overall.

    False.

    The nucleus of an atom has a positive charge due to the presence of positive protons and neutral neutrons.

  • The subatomic particles in the nucleus are known as ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ .

    The subatomic particles in the nucleus are known as ‎ nucleons.

  • The mass of an atom is concentrated in the ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ .

    The mass of an atom is concentrated in the ‎ nucleus.

  • Define atomic number.

    Atomic number is the number of protons.

  • Define mass number.

    Mass number is the number of protons and neutrons.

  • How do you calculate the number of neutrons in an atom?

    To calculate the number of neutrons in an atom:

    • Number of neutrons = mass number - atomic number

      OR

    • Number of neutrons = mass number - number of protons

  • How do you determine the number of electrons in an atom?

    The number of electrons in an atom is the same as the number of protons / the atomic number.

  • Calculate the number of protons, neutrons and electrons in an atom of Al presubscript 13 presuperscript 27.

    The number of protons, neutrons and electrons in an atom of Al presubscript 13 presuperscript 27 are:

    • Protons = 13

    • Neutrons = 27 - 13 = 14

    • Electrons = 13

  • True or False?

    Atoms and ions of the same element have the same number of protons.

    True.

    Atoms and ions of the same element have the same number of protons.

  • True or False?

    The symbol used to represent atomic mass is M.

    False.

    The symbol used to represent atomic mass is A.

  • Why are atoms electrically neutral?

    Atoms are electronically neutral because they have the same number of protons and electrons so the positive and negative charges cancel each other out.

  • Calculate the number of protons, neutrons and electrons in a magnesium ion, Mg2+.

    The number of protons, neutrons and electrons in a magnesium ion, Mg2+ is:

    • Protons = 12

    • Neutrons= 12

    • Electrons = 10

  • The symbol used to represent atomic number is ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎ ‎.

    The symbol used to represent atomic number is Z.

  • Identify the number of protons, neutrons and electrons in a oxide ion, O2-.

    The number of protons, neutrons and electrons in a chloride ion, O2- is:

    • Protons = 8

    • Neutrons = 8

    • Electrons = 10

  • What is an isotope?

    An isotope is an atom of the same element containing the same number of protons but different numbers of neutrons.

  • Which of the following are isotopes?

    • straight C presubscript 6 presuperscript 13

    • straight C presubscript 6 presuperscript 14

    • straight N presubscript 7 presuperscript 14

    The isotopes are straight C presubscript 6 presuperscript 13 and straight C presubscript 6 presuperscript 14.

    straight N presubscript 7 presuperscript 14 is not an isotope because it is a different element (nitrogen not carbon).

  • State two pieces of information required to calculate the relative atomic mass of an element.

    Two pieces of information required to calculate the relative atomic mass of an element are:

    • The mass numbers of each isotope.

    • The (relative / percentage) abundances of each isotope.

  • State the equation for Ar in terms of the percentage abundance and mass of isotopes A and B.

    The equation for calculating relative atomic mass in terms of the percentage abundance and mass of isotopes A and B is:

    fraction numerator left parenthesis percent sign space of space isotope space straight A space straight x space mass space of space isotope space straight A right parenthesis space plus space left parenthesis percent sign space of space isotope space straight B space straight x space mass space of space isotope space straight B right parenthesis over denominator 100 end fraction

  • True or False?

    The relative atomic mass of an element can be calculated using the atomic numbers and relative abundances of all its isotopes.

    False.

    The relative atomic mass of an element is calculated using the mass numbers and relative abundances of all its isotopes.

  • In terms of isotopes, what is abundance?

    In terms of isotopes, abundance is the amount of each isotope present in a sample of an element.

  • True or False?

    Relative atomic mass is calculated by adding the mass numbers of all isotopes.

    False.

    Relative atomic mass is calculated by:

    • Multiplying the abundance of each isotope by its mass

    • Adding these numbers together

    • Then, dividing this value by the total abundance.

  • How can you recognise isotopes from their chemical symbol?

    Isotopes have the same symbol and same atomic numbers but different mass numbers.

  • After calculating the Ar, how would you identify an element?

    After calculating the Ar, you would identify an element by looking for the value on the Periodic Table.

    For example, Ar = 23. On the Periodic Table, the element with an Ar of 23 is sodium.

  • Calculate the relative atomic mass of an element using this information about its isotopes:

    • Isotope 1: Mass = 71, abundance = 39%

    • Isotope 2: Mass = 69, abundance = 61%

    The relative atomic mass of the element is:

    fraction numerator open parentheses 71 cross times 39 close parentheses plus open parentheses 69 cross times 61 close parentheses over denominator 100 end fraction = 69.8 or 70

  • True or False?

    Isotopes display different chemical characteristics.

    False.

    Isotopes display the same chemical characteristics.

  • What determines the chemical characteristics of an atom?

    The chemical characteristics of an atom are determined by the number of electrons in the outer shell.

  • What is a mass spectra used for?

    Mass spectra is used to determine the relative atomic mass of an element from its isotopes.

  • True or False?

    The element has a relative atomic mass between 71 and 72.

    Bar graph showing relative abundance versus mass-to-charge ratio (m/e) with peaks at 70, 71, and 72 m/e. The highest peak is at 71 m/e.

    False.

    The as a relative atomic mass between 70 and 71 because there is a greater abundance of the isotope with a mass of 70 than 72.

    Bar graph showing relative abundance versus mass-to-charge ratio (m/e) with peaks at 70, 71, and 72 m/e. The highest peak is at 71 m/e.

  • Use the mass spectrum to calculate the relative atomic mass of the element.

    Mass spectrum graph showing relative abundance (%) versus m/z (mass-to-charge ratio). Peaks at m/z 121 with abundance 57.2% and m/z 123 with abundance 42.8%.

    The relative atomic mass of the element is:

    Ar  = begin mathsize 14px style fraction numerator left parenthesis 121 space cross times space 57.2 right parenthesis space plus space left parenthesis 123 space cross times space 42.8 right parenthesis space over denominator 100 end fraction end style = 121.9

  • Calculate the relative atomic mass of boron using its mass spectrum.

    Bar graph displays isotopic abundance with m/e on x-axis. Two bars marked 10 (19.9%) and 11 (80.1%) represent different isotopes. Y-axis labeled % abundance.

    The relative atomic mass of boron is:

    fraction numerator open parentheses 19.9 cross times 10 close parentheses plus open parentheses 80.1 cross times 11 close parentheses over denominator 100 end fraction equals space 10.8

  • The mass spectrum of an element is shown below.

    How many isotopes are present in this sample?

    Bar graph showing relative abundance versus mass-to-charge ratio (m/e) with peaks at 70, 71, and 72 m/e. The highest peak is at 71 m/e.

    There are three isotopes present in this sample as there are three peaks.

    Bar graph showing relative abundance versus mass-to-charge ratio (m/e) with peaks at 70, 71, and 72 m/e. The highest peak is at 71 m/e.
Previous:Introduction to the Particulate Nature of MatterNext:Electronic Configurations

    1. Topic 1

      Introduction to the Particulate Nature of Matter

    2. Topic 2

      The Nuclear Atom

    3. Topic 3

      Electronic Configurations

    4. Topic 4

      Counting Particles by Mass: The Mole

    5. Topic 5

      Ideal Gases

    1. Topic 1

      The Ionic Model

    2. Topic 2

      The Covalent Model

    3. Topic 3

      The Metallic Model

    4. Topic 4

      From Models to Materials

    1. Topic 1

      The Periodic Table: Classification of Elements

    2. Topic 2

      Functional Groups: Classification of Organic Compounds

    1. Topic 1

      Measuring Enthalpy Change

    2. Topic 2

      Energy Cycles in Reactions

    3. Topic 3

      Energy from Fuels

    4. Topic 4

      Entropy & Spontaneity

    1. Topic 1

      How Much? The Amount of Chemical Change

    2. Topic 2

      How Fast? The Rate of Chemical Change

    3. Topic 3

      How Far? The Extent of Chemical Change

    1. Topic 1

      Proton Transfer Reactions

    2. Topic 2

      Electron Transfer Reactions

    3. Topic 3

      Electron Sharing Reactions

    4. Topic 4

      Electron Pair Sharing Reactions

    1. Topic 1

      Tool 1: Experimental Techniques

    2. Topic 2

      Tool 3: Mathematics