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CGP Chemistry > Section 2-The Periodic Table and Bonding P1 > Flashcards

Section 2-The Periodic Table and Bonding P1 Flashcards

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1
Q

What is the periodic table?

A

The Periodic Table is a table of all known elements.

-Dmitri Mendeleev ordered the elements by atomic mass to make a table of elements

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2
Q

How is the periodic table arranged?

A

-its laid out in columns (groups) and rows (periods)

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3
Q

What are the features of groups?

A
  • have similar properties

- group number corresponds to the number of electrons in its outer most shell

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4
Q

What are the features of periods?

A

-determines the number of shells an element will have

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5
Q

What are the special names for?
Group 1 elements:
Group 7 elements:
Group 0/8 elements:

A

Group 1 = alkali metals
Group 7 = halogens
group 0/8 = noble gases

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6
Q

How was the periodic table made?

A

The periodic table was made by looking at the properties of the elements and arranging them into groups, the same groups that they have today.

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7
Q

What does the properties of elements depend on?

A

The properties depend on the number of electrons

  • atomic number is therefore significant because it equals the number of electrons
  • the number of electrons in the outer most shell is the most important for chemical properties
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8
Q

What are the electron shell rules:

A
  • electrons always occupy shells, always building from inside out
  • 1st shell has 2 electrons, 2nd and 3rd shell have 8 electrons
  • atoms always try to have full outer shells, but in most atoms the outer shell isn’t full so they want to react to get a full outer shell
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9
Q

How do you work out electronic configurations?

A
  • find out the atomic number
  • start from the inner most shell and fill the with 2 from the atomic number and then carry on for as many electrons you have, adding another shell every 8
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10
Q

How do you draw electronic configurations?

A
  • each circle you surround the nucleus with represents an energy shell and then on each shell you fill it with the number of electrons for that energy level
  • represent electrons with crosses
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11
Q

How do you work out the electronic configuration from its period and group?

A
  • period- tells you the number of shells

- group- tells you the number of electrons in the outermost shell

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12
Q

On the periodic table where is the split between metals and non metals?

A

REMEBER Al-Po B-At

-to the right there is non-metals to the left there is metals

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13
Q

What are general property rules about metals?

A
  • conduct electricity

- metal oxides are basic (they will neutralise acids, they are alkaline)

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14
Q

What are the general property rules for non-metals?

A
  • poor conductors of electricity

- non-metal oxides are acidic (they will neutralise bases, they are acids)

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15
Q

what are the properties on noble gases and why do they have these properties?

A

-they are inert (very unreactive), because they have a full outer shell so they don’t need to gain or loose electrons (they are stable)

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16
Q

Define ions:

A

Ions are charged particles (they can be single atoms or groups of atoms)

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17
Q

Why do atoms gain or loose electrons to form ions?

A

To get a full outer shell

-atoms with full outer shells are stable

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18
Q

Chemical formula for Silver: (and charge)

A

Ag (charge +)

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19
Q

Chemical formula for Iron(II): (and charge)

A

Fe (charge 2+)

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20
Q

Chemical formula for Copper: (and charge)

A

Cu (charge 2+)

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21
Q

Chemical formula for Iron(III): (and charge)

A

Fe (charge 3+)

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22
Q

Chemical formula for Lead: (and charge)

A

Pb (charge 2+)

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23
Q

Chemical formula for Zinc: (and charge)

A

Zn (charge 2+)

24
Q

Chemical formula for Hydrogen: (and charge)

A

H (charge +)

25
Q

Chemical formula for Hydroxide: (and charge)

A

OH (charge -)

26
Q

Chemical formula for Ammonium: (and charge)

A

NH₄ (charge +)

27
Q

Chemical formula for Carbonate: (and charge)

A

CO₃ (charge 2-)

28
Q

Chemical formula for Nitrate: (and charge)

A

NO₃ (charge -)

29
Q

Chemical formula for Sulfate: (and charge)

A

SO₄ (charge 2-)

30
Q

What is ionic bonding between?

A

A non-metal and a metal

31
Q

Describe ionic bonding:

A

The oppositely charge ions are strongly attracted to each other(electrostatic attractions)

  • the non-metal loses electrons(forms a positive ion)
  • the metal gains electrons(forms a negative ion)
32
Q

What is the overall charge of an ionic compound:

A

zero

-all charges must be balance in an ionic compound

33
Q

How do you draw a diagram to represent an ionic compound?

A
  • draw each atom separately, with dots and crosses representing the electrons
  • then draw an arrow and draw the atoms again but this time with the appropriate full outer shell
  • put brackets round the ions and label the charge outside of the brackets
34
Q

Describe the structure of an ionic compound:

A
  • giant ionic structures
  • ions are held together in a closely packed lattice
  • very strong electrostatic attraction
35
Q

Describe the characteristics of an ionic compound:

A
  • very strong electrostatic attraction (so requires a lot of energy to break the bonds - have high melting and boiling points)
  • not electrical conductors as a solid
  • when molten they are electrical conductors (because the electrons are free to move)
36
Q

What is covalent bonding?

A
  • Covalent bonding is when atoms bond together by sharing electrons with other atoms
  • Each covalent bond provides one extra shared electron for each atom
37
Q

Why do atoms bond covalently?

A
  • to feel like they have a full outer shell (makes them stable)
  • strong electrostatic attraction between the negatively charged shared electrons and the positively charged nuclei of the atoms involved
38
Q

What is the bonding in Hydrogen?

A

COVALENT - H₂

-single covalent bond

39
Q

What is the bonding in Chlorine?

A

COVALENT - Cl₂

-single covalent bond

40
Q

What is the bonding in Hydrogen Chloride?

A

COVALENT - HCl

-single covalent bond

41
Q

What is the bonding in Ammonia?

A

COVALENT - NH₃

-made up of three single covalent bonds

42
Q

What is the bonding in Nitrogen?

A

COVALENT - N₂

-one triple covalent bond

43
Q

What is the bonding in Water?

A

COVALENT - H₂O

-two single covalent bonds

44
Q

What is the bonding in Oxygen?

A

COVALENT - O₂

-one double covalent bond

45
Q

What is the bonding in Carbon Dioxide?

A

COVALENT - CO₂

-two double covalent bonds

46
Q

What is the bonding in Methane?

A

COVALENT - CH₄

-four single covalent bonds

47
Q

What is the bonding in Ethane?

A

COVALENT - C₂H₆

-the carbons have one single bond between them and have 3 hydrogen’s each

48
Q

What is the bonding in Chloromethane?

A

COVALENT - CH₃Cl

-four single covalent bonds, one to each hydrogen and chlorine from the carbon

49
Q

What is the bonding in Ethene?

A

COVALENT - C₂H₄

-one double covalent bond between the carbons and 4 single covalent bonds between the carbons and hydrogens

50
Q

Define a covalent bond:

A

The electrostatic attraction between a pair of electrons and the nuclei of two atoms

51
Q

Examples of: Giant covalent structures?

A 
All from carbon
Also known as macro molecules
-diamond
-graphite
-fullerenes
52
Q

Properties of diamond?

A

Carbon

  • all 4 outer electrons Form covalent bonds
  • 3D structure formed
  • each carbon atoms forms 4 bonds to other carbon atoms
  • no weak intermolecular forces
  • very high melting point
  • very hard and abrasive
  • doesn’t conduct electricity
  • used for cutting tools and diamonds
53
Q

What are the properties of giant covalent structures?

A
  • all the atoms are bonded together by strong covalent bonds
  • lots of strong covalent bonds -> lot of energy to break them -> high melting and boiling points
  • don’t conduct electricity (except for graphite when molten)
  • usually insoluble in water
  • made of carbon
54
Q

Properties of graphite?

A

Carbon

  • 3 outer electrons used to form covalent bonds(the fourth becomes a delocalised electron)
  • layered structure formed
  • weak intermolecular forces between the layers
  • high melting point
  • soft and slippery
  • conducts electricity(because of the delocalised electron)
  • used lubricant, pencils
55
Q

What are the properties of simple molecular substances?

A
  • the atoms within a molecule are held together by strong covalent bonds but between the molecules there are weak intermolecular forces
  • low melting and boiling points, easily separated
  • liquid or gas a room temperature generally
  • don’t conduct electricity
  • insoluble in water but soluble in organic solvents
56
Q

As the Mr (relative atomic mass) of a substance increases what happens to the intermolecular forces between the molecules?

A

As the Mr increases the intermolecular forces become stronger because more energy is needed to the intermolecular forces because there are more of them
-melting and boiling points of simple molecular substances increases as the Mr does

57
Q

Properties of Fullerene?

A

C₆₀ is a simple molecular substance

  • hollow sphere structure
  • made up of large covalent molecules
  • Fullerene molecules are held together by intermolecular forces so they can slide over each other
  • has one delocalised electron but it can’t move between the molecules so it’s a poor conductor of electricity

CGP Chemistry (14 decks)

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