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MED 102- GENERAL CHEMISTRY > 6. IONIC BONDING > Flashcards

6. IONIC BONDING Flashcards

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1
Q
  1. What is a Qualitative form of a chemistry law?
A
  • it is a law that is written out in words
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2
Q
  1. What is a Quantitative form of a chemistry law?
A
  • it is a law that is written in the form of a chemical formula
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3
Q
  1. What is the scientific definition for Coloumb’s Law?
A
  • Two point charges in free space or air exert a force on each other.
  • The force is directly proportional to the product of the charges
  • and inversely proportional to the square of the the distance between the charges
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4
Q
  1. How can Coulomb’s Law be described simply?
A
  • like charges repel each other
  • opposite charges attract each other
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5
Q
  1. What is the formula for Coulomb’s Law?
A
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6
Q
  1. What do each of the components in this formula represent?
A
  • R= r1+r2
  • it is the distance between the centres of the ions
  • k is a constant
  • it does not vary across different situations
  • Q1 and Q2 are the charges on the ions
  • if Q1 is positive and Q2 is negative
  • their product will be negative
  • we get a negative E
  • this just means that the interaction is one of attraction
  • if Q1 and Q2 are both either positive or negative
  • their product will be positive
  • we get a positive E
  • this means that the interaction is one of repulsion
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7
Q
  1. What are compounds made up of?
A
  • they are made up of atoms or ions that are joined together by chemical bonds
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8
Q
  1. What does Ionic bonding consist of?
A
  • it consists of two ions joining together
  • it is the force of attraction between negative and positive ions
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9
Q
  1. What does Covalent Bonding consist of?
A
  • it involves neutral atoms joining together
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10
Q
  1. What does the electronic configuration of an atom affect?
A
  • it affects the chemical behaviour of the atoms
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11
Q
  1. Which group of atoms are chemically stable?
A
  • Group 8/8A
  • Noble gases
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12
Q
  1. Are Group 8/8A elements chemically inert?
    Why?
A
  • yes, they are
  • they have s2p6 valence shell electrons
  • this means that they have a full outer shell (an octet)
  • they have no need to either give or take electrons
  • this octet shell gives them the stability to have no need to chemically react
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13
Q
  1. What is the Octet Rule?
A
  • elements react by either taking or giving electrons until they have a full outer shell (an octet)

AN OCTET= s2p6

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14
Q
  1. Explain how Sodium and Chlorine atoms assist one another in becoming stable?
A
  • the Na atoms gives it’s extra electron to the Cl atom
  • now both Na and Cl have a s2p6 outer shell configuration
  • they have followed the octet rule
  • now they are both stable
  • Na will become a Na+ ion as it has lost an electron
  • Cl will become a Cl- ion as it has gained an electrons
  • the two ions are now oppositely charged
  • they attract to each other
  • all the ions join together to form a large crystal lattice
  • this forms the NaCl compound (salt)
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15
Q
  1. What are the Key words for ionic bonding?
A
  • transfer of electrons
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16
Q
  1. Explain the process for the Ionic Bonding of Magnesium and Oxygen?
A
  • the Magnesium atom has two 3s outermost electrons
  • it loses two electrons to gain a s2p6 outer shell electron configuration
  • it now has a full n=2 shell
  • it has followed the octet rule and is stable
  • the Oxygen atom has 6 outermost electrons in the n=2 shell
  • it gains two electrons from Magnesium to fill its n=2 shell
  • it now has 8 electrons in the n=2 shell
  • it has followed the octet rule and is stable
  • Mg is now positively charged
  • this results in an Mg 2+ ion
  • Oxygen is now negatively charged
  • this results in an O 2- ion
  • through Coulombic attraction of opposite charges
  • the Mg 2+ ion is attracted to the O 2- ion
  • the 2 + and the 2 - cancel out
  • this leaves us with the MgO crystal lattice
17
Q
  1. Explain the Ionic Bonding that occurs between Magnesium and Chlorine?
A
  • the Mg atom needs to shed 2 electrons to have a full n=2 shell
  • each Cl atom needs to gain one electron to have a full n=3 shell
  • Mg gives one electron to one Cl atom and and another electron to another Cl atom
  • this results in the Mg atom becoming an Mg2+ ion
  • and the Cl atoms becoming Cl- ions
  • this results in the formula: MgCl2
18
Q
  1. What is a Crystal Lattice?
A
  • it is the alternate arrangements of positive and negative ions
  • ions are arranged in three dimensions
  • ions are crystalline compounds
  • there is an ionic bond between the positive and the negative ions
  • this arrangement forms a solid crystal (salt)
19
Q
  1. Between which two elements do ionic bonds form?
A
  • between metal and non metals
20
Q
  1. What does an increase in the number of ions in a solution of water result in?
A
  • the water has a higher electrical conductivity
  • the electrolytes are stronger
21
Q
  1. What does the strength of the ionic bonds depend on?
A
  • Coulomb’s law
22
Q
  1. What increases lattice energy?
A
  • an increase with the charge on the ions
  • a decrease in the size of the ions also leads to an increase in lattice energy
23
Q
  1. Why is there a decrease in lattice energy from NaF to NaI?
A
  • the ionic charges are the same
    (Na= +1) (halogens= -1)
  • the only thing that varies is the distance between the ions
  • the halogens increase in size as we go down the group
  • the distance (d12) increases as we go down the group
  • this leads to the lattice energy (E) decreasing
24
Q
  1. Why is the lattice energy in MgO four times greater than the lattice energy in NaF?
A
  • the charges in MgO are +2 and -2
  • the product of these two charges is -4
  • the charges in NaF are +1 and -1
  • the product of these two charges is -1
  • negative 4 is four times greater than negative 1
  • therefore the lattice energy will be approximately 4 times greater for MgO than it is for NaF
25
Q
  1. Read through the summary.
    Does everything make sense?
A
  • yes

MED 102- GENERAL CHEMISTRY (27 decks)

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