100% satisfaction guarantee Immediately available after payment Both online and in PDF No strings attached
Previously searched by you
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$15.48
Add to cart
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
2 views 0 purchase
Course
PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1
Institution
PEARSON EDEXCEL GCE A LEVEL CHEMISTRY PAPER 1
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 AL...
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
, 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
3
Turn over
, - 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
4
The benefits of buying summaries with Stuvia:
Guaranteed quality through customer reviews
Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.
Quick and easy check-out
You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.
Focus on what matters
Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!
Frequently asked questions
What do I get when I buy this document?
You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.
Satisfaction guarantee: how does it work?
Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.
Who am I buying these notes from?
Stuvia is a marketplace, so you are not buying this document from us, but from seller ESCALITothethinker. Stuvia facilitates payment to the seller.
Will I be stuck with a subscription?
No, you only buy these notes for $15.48. You're not tied to anything after your purchase.
