Atom, bonding and groups past paper corrections Flashcards Preview

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Flashcards in Atom, bonding and groups past paper corrections Deck (19)
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1
Q

What is the relative mass of an electron?

A

0.0005

2
Q

What is the relative energy between the s orbitals and the p orbitals?

A

The p orbitals have greater energy than the s orbitals

3
Q

What is the definition of molecular formula?

A

The actual number of atoms of each element that make up a molecule

4
Q

How do Van der Waals forces arise between halogens?

A
  • There is an uneven distribution of electrons
  • This creates an instantaneous dipole
  • This causes an induced dipole on a neighbouring halogen
  • This creates a London force
5
Q

Why do boiling points increase down group 7 (halogens)?

A

Br has more electrons than Cl so it can form more London forces
This is stronger so requires more energy to break them

6
Q

What is a repeating pattern of properties in the periodic table called?

A

Periodicity

7
Q

How are there differences in melting points in metallically bonded compounds?

A

eg. Na and Mg
- There are more outer electrons in Mg
- Therefore the Mg IONS have a greater CHARGE density
- So there is a greater attraction between ions and delocalised electrons

8
Q

What is the compound containing sulfur and fluorine that forms 8 bonds?

A

SF6

Sulfur hexafluoride

9
Q

What is the shape of a molecule that has two bonded pairs and two lone pairs?

A

Non linear

10
Q

How do you work out the relative atomic mass?

A

You times the mass number by the percentage (in decimal form) and then add them all up

11
Q

What is the definition of relative atomic mass?

A

The mean mass of an atom compared to 1/12th of the mass of carbon 12

12
Q

What colour is iodine?

A

Purple in an organic solvent

13
Q

How is a salt formed?

A

A hydrogen ion has been replaced by a metal ion

14
Q

What is the definition of empirical formula?

A

The simplest whole number ratio of atoms present in a compound

15
Q

How many electrons are in the fourth shell?

A

32

16
Q

What is the definition of an ionic lattice?

A

A repeating pattern of oppositely charged ions

17
Q

What is the definition of electronegativity?

A

The ability of a bonded atom to attract a shared pair of electrons in a double bond

18
Q

What type of reaction is carbonate to oxide?

A

Thermal decomposition

19
Q

What is an alkali?

A

A proton acceptor that is soluble and releases OH- ions into a solution