chemistry ionic , covalent flashcards

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1. Card 1

   Define ionic bonding and explain how it differs from covalent bonding in terms of electron movement.

   Ionic bonding is the strong electrostatic force of attraction between oppositely charged ions, formed when a metal atom transfers one or more electrons to a non-metal atom. In contrast, covalent bonding involves non-metal atoms sharing pairs of electrons between each other, rather than transferring them.

2. Card 2

   How do metal atoms achieve a full outer shell of electrons when forming an ionic bond?

   Metal atoms achieve a full outer shell by losing electrons to form positive ions (cations). This loss of electrons results in the atom having more protons than electrons, giving it a positive charge and a stable electron configuration similar to a noble gas.

3. Card 3

   Explain why ionic compounds typically have high melting and boiling points.

   Ionic compounds have high melting and boiling points due to the strong electrostatic forces of attraction between the oppositely charged ions in their giant ionic lattice structure. A significant amount of energy is required to overcome these strong forces and break down the lattice.

4. Card 4

   Describe the formation of a chloride ion (Cl-) from a chlorine atom, including the change in electron count and charge.

   A chlorine atom, being a Group 7 non-metal, gains one electron to achieve a full outer shell. This gain of an electron results in the formation of a negative chloride ion (Cl-), as it now has one more electron than protons.

5. Card 5

   Why are intermolecular forces not considered chemical bonds?

   Intermolecular forces are not considered chemical bonds because they do not involve the transfer or sharing of electrons, and no new compounds are formed. They are typically much weaker, around one-tenth the strength of a chemical bond.

6. Card 6

   How does the group number of an element relate to the charge on the ion it forms in an ionic bond?

   The group number of an element directly relates to the charge on the ion it forms. For example, Group 1 metals form 1+ ions, Group 2 metals form 2+ ions, Group 6 non-metals form 2- ions, and Group 7 non-metals form 1- ions, as they gain or lose electrons to achieve a noble gas electronic structure.

7. Card 7

   Explain the primary limitation of a 3D ball and stick model when representing an ionic lattice structure.

   A primary limitation of the 3D ball and stick model is that it incorrectly depicts space existing between individual ions, representing ionic bonds as sticks. In reality, an ionic bond is an electrostatic force of attraction that acts in all directions around an ion, and there is not much space between separate ions.

8. Card 8

   Why do simple covalent molecules not conduct electricity?

   Simple covalent molecules do not conduct electricity because they do not contain free electrons or ions that are able to move and carry an electric charge. The electrons are held in fixed positions within the covalent bonds.

9. Card 9

   What is the role of delocalised electrons in metallic bonding?

   In metallic bonding, delocalised electrons are electrons from the outer shells of metal atoms that are free to move throughout the entire metallic lattice structure. They form a 'sea of electrons' which creates strong electrostatic attractions with the positive metal ions, holding the structure together.

10. Card 10

    Distinguish between bonding electrons and non-bonding electrons in a covalent molecule.

    Bonding electrons are the pairs of electrons that are shared between two atoms to form a covalent bond. Non-bonding electrons, also known as lone pairs, are electrons on the outer shell of an atom that are not involved in forming covalent bonds.

11. Card 11

    How does an atom achieve a greater level of stability by combining with other atoms?

    Atoms combine with other atoms by gaining, losing, or sharing electrons to achieve a full outer shell of electrons. This electron configuration, similar to that of noble gases, represents a state of greater stability for the atom.

12. Card 12

    What are cations and anions, and how are they formed?

    Cations are positive ions formed when atoms lose electrons, resulting in more protons than electrons. Anions are negative ions formed when atoms gain electrons, resulting in more electrons than protons. Both processes occur to achieve a full outer shell.

13. Card 13

    Describe the structure of an ionic compound.

    An ionic compound consists of a giant structure of ions, specifically a regular arrangement of alternating positive and negative ions in a tightly packed lattice. Strong electrostatic forces of attraction between these oppositely charged ions act in all directions, holding the entire lattice together.

14. Card 14

    What is the empirical formula, and how can it be deduced from a dot-and-cross diagram?

    The empirical formula of a compound shows the simplest whole number ratio of atoms of each element present. It can be deduced from a dot-and-cross diagram by counting the atoms of each element, writing their ratio, and then simplifying it to the smallest whole numbers.

15. Card 15

    How does the formation of polyethene exemplify a polymer?

    Polyethene exemplifies a polymer because it is a very large molecule made from many smaller repeating units (ethene monomers) joined together by covalent bonds. This continuous chain of repeating units forms a giant covalent structure.

16. Card 16

    What are the advantages and disadvantages of using dot and cross diagrams to represent chemical bonds?

    Advantages of dot and cross diagrams include illustrating the sharing or transfer of electrons and indicating the origin of bonding electrons. Disadvantages are their failure to illustrate 3D arrangements of atoms and electron shells, and they do not indicate the relative sizes of atoms.

17. Card 17

    Explain why magnesium forms a 2+ ion and oxygen forms a 2- ion when they react to form magnesium oxide (MgO).

    Magnesium is a Group 2 metal, so it loses two outer electrons to achieve a full outer shell, forming a Mg2+ ion. Oxygen is a Group 6 non-metal, so it gains two electrons to achieve a full outer shell, forming an O2- ion. These oppositely charged ions then attract through electrostatic forces.

18. Card 18

    How do the strong electrostatic forces of attraction in an ionic lattice differ from the weak intermolecular forces in simple covalent molecules?

    The strong electrostatic forces in an ionic lattice act between oppositely charged ions throughout the entire giant structure, requiring significant energy to overcome. In contrast, weak intermolecular forces exist only between individual simple covalent molecules, and are much easier to overcome, leading to lower melting/boiling points.

19. Card 19

    What are the three types of bonding studied at GCSE Chemistry?

    The three types of bonding studied at GCSE Chemistry are ionic bonding, covalent bonding, and metallic bonding. These involve the movement of electrons to achieve greater atomic stability.

20. Card 20

    Why is it important to use large square brackets and superscript charges when drawing dot and cross diagrams for ionic compounds?

    Using large square brackets around each ion in a dot and cross diagram for ionic compounds shows that the electrons have been transferred, and the charge is spread evenly across the ion. The superscript charge outside the brackets clearly indicates the overall charge of the ion formed after electron transfer.

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