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Chemistry > 1.1 - Periodic Table > Flashcards

1.1 - Periodic Table Flashcards

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1
Q

What is electronegativity

A

An elements ability to attract electrons often referred to as simply the ‘pulling power’ of an atom, also known as affinity

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2
Q

What is the most electronegative element

A

Fluorine

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3
Q

lowest to highest electronegative elements

A

Metals -> metalloids -> non-metals

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4
Q

What are oxides

A

compounds that contain oxygen

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5
Q

How do you determine the reactivity of oxides

A

Can be determined based on the elements position on the periodic table

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6
Q

What are the acidic oxide reaction types

A

1) React with bases, usually Hydroxide ions

2) Reacts with water

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7
Q

What are acidic oxides

A

Oxides of non-metals, or elements with high electronegativity

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8
Q

Write the chemical reaction with hydroxide ions

A

Acidic oxide + Hydroxide ion ——> Oxyanion + water

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9
Q

What is an oxyanion

A

a negatively charged ion of the element combined with oxygen (o-)

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10
Q

Write the chemical reaction for sulphur dioxide

A

SO2 + 2OH- ——> SO23- + H2O

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11
Q

What is an oxyacid

A

when the acidic oxide reacts and dissolves in water

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12
Q

What is a basic oxide

A

Oxides with metal elements or those with low electronegativity. these compounds are ionic

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13
Q

What are the two basic oxide reactions

A

1) React with acids, usually hydrogen ions

2) reacts with water

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14
Q

Draw the basic oxide reacting with hydrogen ions

A

basic oxide + hydrogen ions —–> metal ion + water

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15
Q

Write the chemical reaction of Copper (II) oxide

A

CuO + 2H+ ——> Cu2+ + H2O

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16
Q

Write the basic oxide reacting with water

A

Basic oxide + water —–> metal ions + Hydroxide ions

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17
Q

Write the chemical reaction of Sodium Oxide

A

Na2O + H2O ——> 2Na+ + 2OH-

18
Q

What is an Amphoteric oxide

A

Can react as other a basic oxide or acidic oxide, depends on the species it is reacting with
Do not react with water

19
Q

In an amphoteric reaction, what will the oxide be if it reacts with Hydroxide ions

A

an acidic oxide

20
Q

In an amphoteric reaction, what will the oxide be if it reacts with Hydrogen ions

A

a basic oxide

21
Q

What is a molecule

A

an element or compound of non-metallic atoms

22
Q

What is classed as a small molecule

A

A molecule that contains 10 or less atoms

23
Q

What are the exceptions for molecules

A

Silicon dioxide, diamond and silicon carbide

these are not molecular. These exhibit continuous lattice structure

24
Q

Properties of molecules

A
  • Low Mp/Bp (can be determined by the attraction between molecules)
  • usually glass or liquids
  • poor conductors of electricity
25
Q

What is covalent bonding

A

describes the bond between atoms in the molecule, known as intramolecular or primary bonds
is the electrostatic attraction of the positive nucleus and the shared electrons
These bonds are very strong

26
Q

What are intermolecular bonds

A 
Also known as secondary bonds
These occur between neighbouring molecules 
Responsible physical properties 
Weaker than intramolecular forces 
These bonds hold molecules together
27
Q

What are the 3 intermolecular forces

A
  • Dispersion forces
  • Dipole - Dipole interactions
  • Hydrogen bonding
28
Q

Draw the molecular shape of PO43- using the VSPER theory

A

Because PO43- contains 3 negatively charged oxygen ions, therefore Phosphate will create 3 single bonds with o- and a double bond with the oxygen atom

29
Q

How many bonds can O- make when drawing a molecule using the VSPER theory

A

1

30
Q

Hydrogen bonding

A
  • Strongest intermolecular bond

- A hydrogen must be bonded to a Nitrogen, Oxygen or Fluorine atom

31
Q

What happens to the polarity of the molecule if it has symmetrical distribution

A

It becomes a non-polar bond overall. Even if it contains polar bonds

32
Q

What happens to the polarity of the molecule if it does not have symmetrical distribution

A

It is a polar bond overall because the bond polarities do not cancel eachother out and therefore there is an uneven distribution of charge in the molecule

33
Q

Dipole - Dipole interactions

A
  • occurs between molecules that have permanent dipoles (ie. polar bonds)
34
Q

What is a polar covalent bond

A

when atoms with different electronegativities are bonded together
These atoms are identified as having partial positive (delta +) or partial negative (delta -) charge
These are dipole bonds

35
Q

Dispersion forces

A
  • the attraction of one molecules nuclei to neighbouring molecules
  • determines whether the compound is solid, liquid or gas
  • For non-polar substances, this is the only secondary force between molecules
  • creates temporary induced dipole - dipole in neighbouring molecules
36
Q

What is the strength of dispersion forces influenced by

A
  • Molar mass, more protons and electrons leads to greater attraction
  • shape, affects how close the molecules can approach one another
37
Q

Why must hydrogen be bonded to Fluorine, Oxygen or Nitrogen to form a hydrogen bond

A

When these elements are bonded to hydrogen, it leaves hydrogen exposed or unsheilding (ie. exposed proton) This strongly attracts the delta - nitrogen, oxygen or fluorine in neighbouring dipoles

38
Q

What does the small size of a Hydrogen atom allow in hydrogen bonding

A

Allows it to come into contact with the delta- atoms of other molecules

39
Q

Distinguish the difference between a linear, v-shaped, trigonal planer, trigonal pyramid and a tetrahedral shaped molecule and give examples

A 
Linear = CS2 
V-shaped = SCl2
Trigonal Planer = HNO2
Trigonal pyramid = NI3 
Tetrahedral SiCl4
40
Q

Identify the s, p, d, f blocks on the periodic table

A

refer to diagram

41
Q

name the three elements which can expand its octet

A

Phosphorus, chlorine and sulphur

Chemistry (6 decks)

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