chemistry chapter 4 bonding Flashcards

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1
Q

what is ionic bonding

A

a strong electrostatic attraction between oppositely charged ions

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2
Q

how are ions formed

A

an atom becomes an ion when it gains or loses electrons

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3
Q

how are positive ions formed

A

when an atom loses electrons, it has less electrons than protons forming a positive ion, also known as cation. Therefore, positive ions or cations are formed when an atom loses electrons

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4
Q

how are negative ions formed

A

when an atom gains electrons, it has more electrons than protons forming a negative ion also known as anions. Therefore negative ions or anions are formed when they gain electrons.

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5
Q

how are ionic compounds formed

A

when a metal reacts with a non metal, the metal atoms transfer their outer electrons to the non metal atoms forming cations and anions

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6
Q

what are the physical properties of ionic compounds

A
  • are crystalline solids
  • have high melting and boiling points
  • have a good electrical conductivity when molten or in aqueous solution
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7
Q

what is a giant lattice structure

A

a three dimensional network of ions. the ions are held in place by ionic bonds and are packed in a regular and a repeating pattern. The giant lattice structure is held tightly because oppositely charged ions attract one another strongly

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8
Q

what is a covalent bond

A

when non metallic elements react with one another, they share electrons in order to achieve the noble gas electronic configuration

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9
Q

covalent bonds can be formed between

A

atoms of the same element and different elements

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10
Q

what are the physical properties of simple molecules

A
  • have low melting and boiling points
  • are poor electrical conductors
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11
Q

what are the physical properties of giant covalent substances

A
  • high melting and boiling points
  • do not conduct electricity except graphite
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11
Q

what is a giant covalent structure

A

a three dimensional regular arrangement of atoms or molecules joined by strong covalent bonds

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12
Q

give an example of a giant covalent structure

A

diamonds and graphite

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12
Q

why do giant covalent substances have high melting and boiling points

A

a giant covalent structure consists of a large number of atoms that are held together by strong covalent bonds. To melt or boil these substances, the strong bonds must be broken. This requires a lot of energy meaning that these substances will have high melting and boiling points making them solids at room temperature

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13
Q

why do giant covalent substances not conduct electricity

A

in giant covalent substances, all the outer electrons of atoms are used to form covalent bonds, Thus, there are no delocalised electrons that move through the structure to conduct electricity

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14
Q

what is metallic bonding

A

electrostatic attraction between the positive ions in a giant metallic lattice and a ‘sea’ of delocalised electrons.

15
Q

why does metals conduct electricity

A

Metals conduct electricity. Delocalised electrons move to the positive terminal. Electrons are negatively charged meaning that electrons will only be attracted to positively charged ions, also known as protons. This is because oppositely charged ions are attracted to each other.

15
Q

before force is applied, how are the metal ions arranged

A

before force is applied, the metal ions form an orderly and rigid arrangement

16
Q

what happens to the metal ions when force is applied

A

when force is applied, one layer of metal ions slide over the other through the ‘sea’ of delocalised electrons

17
Q

what is the effect of a force on the metallic lattice

A

They layers of metal ions can slide over one another. The metal is malleable

18
Q

why are alloys harder and stronger than pure metals

A

The layers or metal ions cannot slide as easily over one another, because large metal ions are disrupting the regular lattice.