Combined

• What are the terms of the Atomic Theory?

  •All matter is made up of tiny particles called atoms

  •Atoms are tiny, hard spheres that cannot be broken down into smaller parts

  •Atoms cannot be created or destroyed

  •The atoms in an element are all identical (but each element has its own type of atom).
• Name the subatomic particles.

  electrons, protons, and neutrons
• What is the relative charge and mass of a proton?

  +1, 1
• What is the relative charge and mass of an electron?

  -1, 0.0005 (zero)
• What is the relative charge and mass of a neutron?

  0, 1
• Why do atoms in elements have no overall charge?

  They always have an equal number of protons and electrons so the charges cancel out.
• Name a pro and con for models of atoms.

  •They help us to understand their structure.

  •But most don't give us a correct impression of the scale. The overall diameter of an atom can be 100,000 times the diameter of its nucleus.
• Recall Ernest Rutherford's experiment on the structure of atoms.

  Positive particles were fired at a thin gold foil. Most of the particle's passed straight through the gold foil, with a few being deflected and a very small number bouncing back.
• What was Ernest Rutherford's conclusion?

  He suggested that atoms are mostly empty space, with a small positive central nucleus that contains most of the mass.
• How were elements in the periodic table originally organised?

  In order of the masses of their atoms.
• What was wrong with this order?

  It caused some elements to be grouped with others that had very different properties.
• How did they try to resolve this?

  A few elements were swapped round to make sure that those with similar properties were grouped together, even if it meant that they were no longer in the correct order of mass.
• How did Henry Mosley contribute to the periodic table?

  He confirmed that the rearranged order of elements in the table was actually correct- he showed that they were in the order of the amount of positive charge in the nucleus.
• How does the modern periodic table place the elements?

  In order of the number of protons in their atoms.
• What is atomic number?

  The number of protons in an atom. All of the atoms of a particular element have the same unique atomic number.
• What is mass number?

  The total number of protons and neutrons in a nucleus.
• Why doesn't the number of electrons affect the mass of an atom?

  The mass of an atom is described as "negligible"- it is so small that it can be ignored.
• What are isotopes?

  Atoms containing the same amount of protons and electrons but different amounts of neutrons. Therefore, such atoms have the same atomic number but different mass numbers.
• How can we refer to a specific isotope?

  By adding its mass number to the element's name.
• What is relative atomic mass?

  The mean mass of an atom relative to (compared to) the mass of an atom of carbon-12, which has a mass of exactly 12. Carbon-12 is used as a standard.

  The RAM of an element is the mean relative mass of the isotopes in the element.
• What is the relative mass of an isotope?

  Its mass number.
• How to find the relative atomic mass?

  •Mass number of each isotope multiplied by its abundance. Calculate the total mass of its atoms.

  •Divide the total by 100.

  •Round to 1 decimal point.
• What is an ionic bond?

  A strong electrostatic force of attraction between oppositely-charged ions.
• What are bonds?

  Forces of attraction that hold atoms together.
• How do atoms become stable?

  By losing or gaining electrons. This can happen by the transfer of electrons between atoms.
• What are the most stable atoms?

  Noble gases. Because they have full outer electron shells.
• What are ions?

  An atom or group of atoms that has an electric charge. Due to the loss or gain of electrons.
• What are cations?

  Metal atoms that have lost electrons and formed positive ions. They have more protons than electrons.
• What are anions?

  Non-metal atoms that have gained electrons and formed negative ions. They have more electrons than protons.
• What are electrostatic forces?

  Forces of attraction between all positively and negatively charged objects. These forces hold the oppositely charged ions together.
• What kind of atoms easily form ions?

  Atoms with a nearly full or a nearly empty outer electron shell.
• What are ionic bonds mostly formed between?

  A metal and a non-metal.
• What does an ion being formed depend on?

  The element's position in the periodic table and its number of outer electrons.
• What are ionic compounds?

  They are formed by the loss and gain of electrons, held together by strong electrostatic forces of attraction between oppositely charged ions. These strong ionic bonds allow 'billions' of ions to be packed together in a regular repeating arrangement called a LATTICE STRUCTURE
• What will ionic compounds form when solid?

  Crystals because of their regular lattice structure.
• What are crystals?

  Pieces of solid that have a particular regular shape, flat surfaces and sharp edges.
• What charge do ionic compounds have?

  Electrically neutral (they have no overall charge).
• Why do ionic compounds have high melting and boiling points?

  The electrostatic forces of attraction between oppositely charged ions are strong. A lot of energy is needed to overcome these forces in order to separate the ions and cause the substance to melt. This is why ionic compounds must be heated to high temperatures before they change state. They have high melting and boiling points.
• Why do ionic compounds have high melting points?

  Some ions have more than 1 charge. These highly charged ions will attract other ions more strongly than ions with one charge. More energy will be needed to overcome the electrostatic forces of attraction and so the melting points will be higher.
• When and why do ionic compounds conduct electricity?

  When molten or dissolved in water. Because the ions are free to move and so it does conduct electricity.