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LGS GCSE OCR Chemistry A - Aayan 😎 > C2.2 - Bonding > Flashcards

C2.2 - Bonding Flashcards

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1
Q

What are typical properties of metals?

A
  • Shiny
  • Usually high MP and BP
  • Solid (apart from mercury)
  • Malleable
  • Ductile
  • Good conductors
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2
Q

What are typical properties of non-metal elements?

A
  • Dull
  • Usually low MP and BP
  • About half are solid and half are gas at room
    temperature
  • Brittle
  • Non-ductile
  • Poor conductors
  • Insulators
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3
Q

How can metals and non metals be separated on the periodic table?

A

They can be separated by a zigzag boundary starting from under Boron.

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4
Q

What are chemical properties of a substance?

A

A chemical property is a characteristic of a substance that can only be determined by studying its chemical reactions.

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5
Q

What are two chemical properties of metals and non metals?

A
  • Metals lose electrons to form positive ions, but
    non- metal atoms gain electrons to form negative
    ions.
  • Metal oxides produce alkaline solutions if
    dissolved in water.
  • Non-metal oxides produce acidic solutions if
    dissolved in water.
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6
Q

What does the electron structure of an element show?

A

The electronic structure of an element shows how the electrons are arranged in atoms.

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7
Q

What is the outer shell?

A

The outermost occupied shell in an atom is called the outer shell.

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8
Q

How is electron structure related to the Periodic Table?

A
  • The last number equals the non-IUPAC group
    number.
  • The number of numbers equals the period
    number.
  • The sum of the numbers equals the atomic
    number.
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9
Q

What is an ion?

A

An ion is a charged particle formed when an atom, or group of atoms, loses or gains electrons.

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10
Q

How do metals and non-metal form ions?

A
  • Metal atoms lose electrons to form positive
    ions.
  • Non-metal atoms gain electrons to form
    negative ions.
  • Non metals and metals gain or lose electrons to
    make a complete outer shell.
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11
Q

What does an electron diagram show and how do you draw one?

A
  • An electron diagram represents the electronic
    structure of an atom or ion.
  • Circle to represent each shell.
  • Dots or crosses to represent its electrons - To also
    represent which electrons are gained.
  • Charge written outside the brackets on the top
    right.
  • Element symbol written in the centre
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12
Q

How do ionic compounds form?

A
  • When a metal reacts with a non-metal, electrons
    are transferred from the metal atoms to the non-
    metal atoms so that they both achieve more stable
    electronic structures.
  • Metal atoms become positively charged and non-
    metals atoms become negative ions.
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13
Q

How can you model ionic compounds?

A
  • You can model the ions in the ionic compounds
    that is formed using a dot-and-cross diagram.
  • Electrons from one atom as dots.
  • Electrons from the other atom as crosses.
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14
Q

What is the structure and bonding in ionic compounds?

A
  • Giant ionic lattice.
  • A structure of ionic compounds in which
    oppositely charged ions are held in a regular and
    repeating arrangement by strong electrostatic
    forces of attraction.
  • Ionic bonding - Strong electrostatic forces of
    attraction between oppositely charged ions.
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15
Q

What are the limitations of a ball-and-stick model representing an ionic compound?

A
  • Ions are actually close together.
  • Bonds are forces rather than physical objects
    made from matter.
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16
Q

What is a covalent bond?

A

A covalent bond is a strong electrostatic force of attraction between the nuclei of two (bonded) atoms and their shared pair(s) of electrons.

17
Q

How can covalent bonds be modelled?

A
  • Using a dot-and-cross diagram.
  • Electrons from one of the bonded atoms are
    shown as dots.
  • Electrons from the other bonded atom are
    shows as crosses
  • Each pair of electrons in the shared area
    between the overlapping circles represent a
    covalent bond.
  • Only outer shells are usually shown.
18
Q

What is a simple molecule?

A

A molecule that contains only a few non-metal atoms covalently bonded.

19
Q

What is the difference between the covalent bonds and the intermolecular forces of a simple molecule?

A
  • Covalent bonds between the atoms in a simple
    molecule are strong.
  • Intermolecular forces between the molecules are
    weak.
20
Q

What are the limitations of a displayed formula of a simple molecule?

A

Simple molecule have shapes, however a displayed formula does not show the three-dimensional shape of the molecule.

21
Q

What is a giant covalent structure?

A

An arrangement of very many non-metal atoms joined by covalent bonds in a regular repeating arrangement.

22
Q

How does diamond exist?

A
  • As having a giant covalent structure.
  • Each carbon atom is joined to four other carbon
    atoms by covalent bonds.
23
Q

How do you write the chemical formula of ionic compounds and giant covalent structures?

A

You use the empirical formula as there are many ions/very many atoms involved and it makes little sense to write a chemical formula with the huge numbers.

24
Q

What is a polymer?

A

A substance with molecules made from many repeat units.

25
Q

What are monomers?

A

Small, simple molecules that can join together in chemical reactions to form polymer molecules.

26
Q

How can you model monomers?

A
  • Dot and cross diagram.
  • Displayed formula.
  • Ball and stick model.
27
Q

What is a thermosoftening polymer?

A
  • Each polymer molecule is drawn as a wavy line
    (in diagram).
  • Weak intermolecular forces.
  • Polymer chains are relatively easy to separate.
28
Q

What is a thermosetting polymer?

A
  • Each polymer molecule is drawn as a wavy line.
  • Cross linking.
  • Chains joined by strong covalent
    bonds.
29
Q

What is the structure of metals?

A
  • All metals apart from mercury are solid at room
    temperature.
  • Their ions are packed together in a regular way,
    forming a giant metallic lattice.
30
Q

What are metallic bonds?

A

Metallic bonds are the strong electrostatic forces of attraction between the delocalised electrons and the closely packed, positively charged nucleus.

31
Q

What are delocalised electrons?

A

The ‘sea’ of electrons around the positively charged metal ions in the structure of a metal.

32
Q

What did Mendeleev consider before making his first table?

A
  • The atomic weights of the known elements, similar
    to our modern relative atomic masses.
  • Knowledge of the chemical reactions of different
    elements.
  • Knowledge of physical properties, such as
    melting points and boiling points
33
Q

How did Mendeleev arrange the elements in his periodic table?

A
  • In order of increasing atomic weight.
  • Grouped together the ones with similar
    chemical properties.
  • Swapped tellurium and iodine because he felt
    that this matched their chemical properties
    better.
  • Left out spaces for elements he though would
    exist but were not yet discovered, and predicted
    their properties from those of nearby elements.
  • Died before proton was discovered.
  • Henry Mosely discovered that an atom’s atomic
    number was actually the number of protons in
    its nucleus.
34
Q

Why did Mendeleev not accept inert gases at first?

A

Mendeleev thought that elements should be able to react with other elements, so he was reluctant to believe that helium and argon were elements.

35
Q

What is electronic structure determined by and what does it determine?

A
  • Electronic structure is determined by the
    number of protons.
  • The electronic structure of an element
    determines its chemical properties.
36
Q

What happens as you go down group 1,2 and 7 of the periodic table?

A
  • Elements in group 1 and two become more
    reactive as you go down the group.
  • Elements in group 7 become less reactive as
    you go down the group.

LGS GCSE OCR Chemistry A - Aayan 😎 (17 decks)

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