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2024 PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1 (9CH0/01) EXAM COMPLETE WITH ACTUAL QUESTIONS AND COMPLETE 100%CORRECT ANSWERS WITH VERIFIED AND WELL EXPLAINEDRATIONALES ALREADY GRADED A+ BY EXPERTS |LATEST VERSION 2024 WITH GUARANTEED SUCCESS AFTER D

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PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1

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PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1

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2024 pearson edexcel gce a level chemistry paper 1
2024 pearson edexcel gce a level chemistry
pearson edexcel gce a level chemistry paper 1

Institution PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1
Course PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1

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2024 PEARSON EDEXCEL GCE A LEVEL
CHEMISTRY PAPER 1 (9CH0/01) EXAM
COMPLETE WITH ACTUAL QUESTIONS
AND COMPLETE 100%CORRECT ANSWERS
WITH VERIFIED AND WELL
EXPLAINEDRATIONALES ALREADY
GRADED A+ BY EXPERTS |LATEST VERSION
2024 WITH GUARANTEED SUCCESS AFTER
DOWNLOAD ALREADY PASSED!!!!!!!
(PROVEN ITS ALL YOU NEED TO EXCEL IN
YOUR EXAMS

, why does first ionisation energy decrease between groups 2 and 3 in group 3 the outermost electrons are in p orbitals whereas in group 2 they are in s orbitals so more easily removed

why does 1 ionisation every decrease between group 5 and 6 group 5 electrons in p orbitals are single electrons. in group 6 outer most electrons are spin paired so there is some repulsion so the
electrons are more easily removed

what happens to first ionisation energy between the end of one period and the start of the next it decreases as there is an increase in atomic radius and an increase in atomic shielding as there is an
additional full shell of electrons

why does first ionisation energy decrease down a group - shielding increases meaning weaker attraction to outer electron

- atomic radius increases, so distance between nucleus and outer electrons increases so less attraction

- increased nuclear charge is outweighed by the increased shielding and atomic radius

ion charged particle that is formed from the loss or gain of electrons

what are the 3 main types of bonds ionic, covalent, metallic

2
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, ionic bonding the electrostatic attraction between positive and negative ions

what determines strength of ionic bond - ionic radius and ionic charge

- ionic bonding is stronger (therefore melting point is higher) when ions are smaller or have higher charge

explain trend in ionic radius down a group Ionic radii increases going down the group. This is because down the group the ions have more shells of electrons and thus the outermost electron
experience less pull from positive nucleus.

physical properties of ionic compounds - high melting points

- non conductor of electricity when solid

- conductors of electricity when in solution or molten

- brittle

covalent bonding electrostatic attraction between a shared pair of electrons and the nuclei

metallic bonding electrostatic attraction between the positive metal ions and the sea of delocalised electrons

Why does giant ionic lattice conduct electricity when liquid but not when solid? in solid state the ions are in fixed positions and so cannot move. when in liquid state the ions are mobile and can
freely carry charge

why do giant ionic lattices have high melting and boiling point a large amount of energy is required to overcome electrostatic bonds

what is the effect of multiple covalent bonds double/triple bonds exert a greater electron density therefore the attraction between nucleus and electron is greater resulting in a shorter and
stronger bond

lone pair electrons in the outer shell that are not involved in the bonding

Dative covalent bond A bond where both electrons in the shared pair belong to the same atom

describe the bonding in simple molecular structures atoms within the same molecule are held by strong covalent bonds and different molecules are held by weak intermolecular forces

Why do simple molecules have low melting points and boiling points? small amount of energy is enough to overcome the intermolecular forces

list some properties of giant covalent structures ● High melting and boiling point

● Non conductors of electricity, except graphite

● Insoluble in polar and non polar solvents

what was stated in dalton's atomic theory ● Atoms are tiny particles made of elements

● Atoms cannot be divided

● All the atoms in a element are the same

● Atoms of one element are different to those of other elements

what did Thompson discover about electrons ● They have a negative charge

● They can be deflected by magnet and electric field

● They have very small mass

explain the current model of the atom -Protons and neutrons are found in the nucleus

-Electrons orbit in shells

-Nucleus is tiny compared to the total volume of atom

-Most of atom's mass is in the nucleus

-Most of the atom is empty space between the nucleus

and the electrons

what is charge on a proton and electron +1 and -1

isotope atoms of the same element with a different number of neutrons but the same number of protons so mass number is different

why do different isotopes of the same element react in the same way - neutrons have no impact on chemical reactivity

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, - reactions involve electrons, isotopes have same electronic configuration

relative atomic mass the weighted mean mass of an element compared to 1/12 the mass of an atom of carbon- 12

relative isotopic mass the mass of an atom of isotope compared to 1/12 the mass of an atom of carbon-12

what are the uses of mass spectrometry ● Identify unknown compounds

● Find relative abundance of each isotope of an element

● Determine structural information

what is a shell A group of orbitals with the same principal quantum number

what is an orbital A region of space around the nucleus that can hold up to two electrons with opposite spins

shape of s orbital and p orbital s- sphere p- dumbell

what are the rules by which electrons are arranged in a shell -electrons are added one at a time

- Lowest available energy level is filled first

- each energy level must be filled before the next one can fill

- each orbital is filled singly before pairing

- 4s is filled before 3d

why is 4s filled before 3d 4s orbital has a lower energy than 3d

how is group number related to electron number group number = number of outer electrons

define periodicity the repeating trends in chemical and physical properties

what change happens across each period elements change from metal to non-metal

first ionisation energy the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous +1 ions under standard conditions

what factors affect ionisation energy - atomic radius

- nuclear charge

- electron shielding

explain trends in this period 3 ionisation energy using the graph - first ionisation energy increases due to increased nuclear charge, decreasing atomic radius and the same electron shielding as all
the elements have the same number of shells.

- this means more energy is required to remove the outer electron.

- dip at Al as the outer electron is in a 3p orbital which has a higher energy than a 3s orbital so less energy required to remove electron

- dip at s as one 3p orbital has 2 electrons, repulsion occurs so less energy to remove one

how does graphite conduct electricity Delocalised electrons present between the layers are able to move freely carrying the charge

Why do giant covalent structures have high melting and boiling points? strong covalent bonds within the molecules need to be broken which requires a lot of energy

what does the shape of a molecule depend on The number of pairs of electrons in the outer shell of the central atom, and the number of the pairs that are bonded or lone pairs

shape and bond angle of 2 bonded pairs, 0 lone pairs linear, 180 degrees e.g CO2

what is the oxidation number of oxygen in H2O -2

what is the oxidation number of oxygen in peroxides -1

what is oxidation number of hydrogen in NH3 or H2S +1

what is oxidation number of hydrogen in metal hydrides e.g LiH -1

What is the oxidation number of a simple ion the charge on the ion

Define oxidation the loss of electrons , gain in oxygen and increase in oxidation number, loss of hydrogen

define reduction loss of oxygen, gain of electrons, decrease in oxidation number, gain of hydrogen

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Exam (elaborations)

2024 PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1 (9CH0/01) EXAM COMPLETE WITH ACTUAL QUESTIONS AND COMPLETE 100%CORRECT ANSWERS WITH VERIFIED AND WELL EXPLAINEDRATIONALES ALREADY GRADED A+ BY EXPERTS |LATEST VERSION 2024 WITH GUARANTEED SUCCESS AFTER D

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