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AS Chemistry Lesson 1 atomic structure

AS Chemistry Lesson 1 atomic structure. Friday, 03 January 2020. Atomic Structure (a) describe protons, neutrons and electrons in terms of relative charge and relative mass; (b) describe the distribution of mass and charge within an atom;

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AS Chemistry Lesson 1 atomic structure

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  1. AS ChemistryLesson 1 atomic structure Friday, 03 January 2020

  2. Atomic Structure (a) describe protons, neutrons and electrons in terms of relative charge and relative mass; (b) describe the distribution of mass and charge within an atom; (c) describe the contribution of protons and neutrons to the nucleus of an atom, in terms of atomic (proton) number and mass (nucleon) number; (d) deduce the numbers of protons, neutrons and electrons in: (i) an atom given its atomic and mass number, (ii) an ion given its atomic number, mass number and ionic charge; (e) explain the term isotopes as atoms of an element with different numbers of neutrons and different masses; Lesson objectives

  3. Remember this is a model. It is the nuclear model of an atom. ELECTRON – negative (-1), mass 1/2000 (so small compared to the nucleus we say it is negligible). Occupy shells around the nucleus Nucleus contains protons and neutrons NEUTRON – neutral (0), same mass as proton (“1”) PROTON – positive (+1), same mass as neutron (“1”) - + + - Draw a labelled diagram for the structure of the atom. This can be any atom or just a generic diagram. Structure of the atom

  4. Essential information

  5. Some GCSE revision questions • The number of protons that an element has determines what atoms it contains. For example, all carbon atoms have six protons. In any atom, which particle is present in the same number as the number of protons?   • Using the properties of the subatomic particles explain why is there no overall charge on an atom?  • Using the properties of the subatomic particles justify where most of the mass of an atom is found.  • Using the structure of an atom determine where most of the matter (material) in an atom is distributed.  • Why is the overall charge of the nucleus positive?

  6. Most of the atom is empty space! If you imagine an atom being the size of Wembley stadium, the nucleus would be about the size of a football on the centre spot. The electrons would be two peas flying around the whole stadium. The rest of it: emptiness.

  7. What is the structure of an atom? Protons, neutrons and electrons are not evenly distributed in an atom. The protons and neutrons exist in a dense core at the centre of the atom. This is called the nucleus. The electrons are spread out around the edge of the atom. They orbit the nucleus in layers called shells. In an atom the number of positive protons is the same as the number of negative electrons.

  8. Nucleus contains protons and neutrons, overall charge is positive. Most of an atoms mass is found here. Most of the atom is empty space. Electrons give the atom it’s overall size and shape. An atom has no overall charge because the number of positive protons is the same as the number of negative electrons.

  9. Distribution of mass in an atom • The nucleus of an atom takes up almost no space • It is tiny but it makes up most of the mass of the atom • This is because it contains protons and neutrons which both have a mass of 1, the electrons orbit the nucleus and have negligible mass • It contains positive protons and neutral neutrons – so it overall it is positive

  10. Distribution of matter in atoms • The rest of the atom is mostly empty space • There are negative electrons going around the nucleus really fast. They give the atom its overall size

  11. The mass of an electron is negligible compared to a proton or neutron, this means you can usually ignore it.

  12. Isotopes The number of protons is what determines which element it is. 8 protons = oxygen 2 protons = helium But the number of neutrons can vary. If the neutrons vary then what else will vary? If neutrons vary then so does the atoms…. ….mass!

  13. Isotopes Definition: • Isotopes are atoms of the same element with different numbers of neutrons. • Isotopes of an element will have: • different masses • the same number of protons and electrons • different numbers of neutrons • Isotopes of an element react in exactly the same way because reactions involve electrons, neutrons have no effect on chemical reactions.

  14. Mass number (nucleon number) total number of protons and neutrons in the nucleus Element symbol X A Z Symbol for an isotope • Atomic (proton) number • Number of protons in the nucleus – defines the element • All atoms of the same element have the same number of protons

  15. Chlorine -35 and -37 are examples of isotopes Different mass numbers mean different numbers of neutrons Cl Cl 37 35 17 17 18 neutrons 20 neutrons (35 – 17) (37 – 17) The atomic numbers are the same. Both isotopes have 17 electrons and 17 protons Remember Number of neutrons = mass number – atomic number

  16. It is the number and arrangement of electrons that decides the chemical properties of an element. Isotopes have the same configuration of electrons, so they have the same chemical properties. • Isotopes of an element do have slightly different physical properties such as density and rates of diffusion, which is dependant on the mass of particles.

  17. Isotopes of Carbon Carbon is a mixture of three isotopes, for each of them complete the table: C C C

  18. Isotope questions (actual exam ones) • Hydrogen, deuterium and tritium are all isotopes of each other. • Identify one similarity and one difference between these isotopes. • Deuterium can be written as 2H. Determine the number of protons, neutrons and electrons in a neutral deuterium atom. • Write a nuclear symbol for tritium, given that it has 2 neutrons. 2. A certain atom X has one less proton and two more neutrons than K. What are its atomic number and mass number? • Explain in terms of sub atom particles, why C-12 and C-14 are isotopes

  19. Ions What is an ion? It is an atom that is charged. How does this happen? Either by gaining or losing one or more electrons. DefinitionAn ion is a positively or negatively charged atom or (covalently bonded) group of atoms (a molecular ion)

  20. Ions • Ions have different numbers of protons and electrons • Negative ions have more electrons than protons e.g. Br- the negative charge means that there’s one more electron than there are protons. Br has 35 protons, so it must have 36 electrons. The overall charge is +35 – 36 = -1

  21. Positive ions have fewer electrons than protons e.g. Mg 2+ charge means that there’s 2 fewer electrons than there are protons. Mg has 12 protons, so Mg 2+ must have 10 electrons. The overall charge = +12 – 10 = +2

  22. Ions Complete the table: Cl- Na+

  23. Ions questions a) How many protons, neutrons and electrons are in the following atoms and ions? b) Which are atoms and ions? How do you know? • 173Li 2) 2411Na 3) 199F 4) 5526Fe 5) 3919 K+ 6) 199 F- 7) 3920 Ca 2+ 8) 178 O 2-

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