Atomic Structure (Edexcel GCSE Chemistry)

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  • What are the key ideas of Dalton's atomic theory?

    The key ideas of Dalton's atomic theory are:

    1. Atoms cannot be created, destroyed, or divided.

    2. Atoms of the same element are identical.

    3. Atoms combine to form new substances.

  • What is an atom?

    An atom is a tiny particle that makes up matter.

  • True or False?

    Different atoms combine together to form new substances.

    True.

    Different atoms combine together to form new substances.

  • When can a scientific model can be changed or replaced?

    A scientific model can be changed or replaced when new experimental evidence improves our understanding.

  • What is the mass and charge of a proton?

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

  • True or False?

    All atoms of the same element have the same number of protons.

    True.

    All atoms of the same element have the same number of protons.

  • What is the 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.

  • 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

  • True or False?

    Atoms are made of subatomic particles.

    True.

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

  • Which subatomic particle has a mass of 1 and a charge of 0?

    The subatomic particle with a mass of 1 and a charge of 0 is the neutron.

  • 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.

  • Why are reason atoms are electrically neutral?

    Atoms are electrically neutral because they have the same number of electrons as protons.

  • 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 nucleus?

    The nucleus is the central part of the atom.

  • Define atomic number.

    The atomic number is the number of protons (in the nucleus of an atom).

  • Define mass number.

    The mass number is the total number of protons and neutrons (in the nucleus of an atom).

  • Where is most of the mass of an atom?

    Most of the mass of an atom is in the nucleus.

  • True or False?

    The nucleus of an atom is roughly half the size of an atom.

    False.

    The nucleus of an atom is very small compared to the overall size of the atom.

  • Which number do atoms of the same element have in common?

    Atoms of the same element have the same:

    • Proton number / number of protons.

    • Number of electrons.

  • True or False?

    The mass number is unique to an element.

    False.

    The atomic number is unique to an element.

  • Why do chlorine and copper not have whole numbers for their atomic mass?

    Cl presubscript 17 presuperscript 35.5 end presuperscript Cu presubscript 29 presuperscript 63.5 end presuperscript

    Elements like chlorine and copper do not have whole numbers for their atomic mass because of isotopes.

  • What is an isotope?

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

  • Calculate the number of protons, neutrons and electrons in straight H presubscript 1 presuperscript 3.

    The number of protons, neutrons and electrons in straight H presubscript 1 presuperscript 3are:

    • Protons = 1

    • Neutrons = 2

    • Electrons = 1

  • How can you find out the number of neutrons in a atom?

    Number of neutrons = mass number - atomic number.

  • How can you recognise isotopes from their chemical symbol?

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

  • 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).

  • 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.

  • How can you find out the number of protons in a neutral atom?

    The number of protons is the atomic (proton) number.

  • What is the difference between isotopes of the same element?

    The difference between isotopes of the same element is the number of neutrons.

  • How can you find the number of electrons in a neutral atom?

    In a neutral atom, the number of electrons is equal to the number of protons, which is the atomic number.

  • Calculate the number of protons, neutrons and electrons in straight C presubscript 6 presuperscript 13.

    The number of protons, neutrons and electrons in straight C presubscript 6 presuperscript 13 are:

    • Protons = 6

    • Neutrons = 7

    • Electrons = 6

  • True or False?

    Mass number and relative atomic mass are the same.

    False.

    Mass number and relative atomic mass are not the same.

    Relative atomic mass is an average of all isotopes.

  • 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.

  • 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

  • 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.

  • 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 = 35, abundance = 75%

    • Isotope 2: Mass = 37, abundance = 25%

    The relative atomic mass of the element is:

    fraction numerator open parentheses 35 cross times 75 close parentheses plus open parentheses 37 cross times 25 close parentheses over denominator 100 end fraction = 35.5