Atomic Structure Chemistry Flashcards
What is a homologous series?
families of organic compounds with the same functional group and same general formula.
Order of priority
Carboxylic acids>aldehydes>ketones>alcohols>alkenes>halogenoalkanes
What is cracking?
The breaking down of alkanes or larger molecules in order to produce smaller molecules to be used in different industries
Define first ionisation energy
the energy required to remove one mole of the most loosely held electrons from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+.
Factors that effect first ionisation energy
Atomic radius-the half distance from the nucleus to the outermost electron
Nuclear charge- the number of protons in the nucleus which attract the outer electrons more
Shielding- the inner electron shells repel the outer electron shells. The more the inner shells increase the weaker the attraction between the nucleus and the furthermost electron decreases
What are orbitals?
regions of space that electrons are likely to occupy and inhabit. They have the notations s,p,d,f.
What is the periodicity for ionic radii in metals?
The size of the ions are smaller than the atom in the beginning as they lose valence electrons but they don’t lose entire shells. The nuclear charge becomes stronger and pulls in the electrons
What is the periodicity for ionic radii in non metals?
The size of the ions are bigger than the atom in the beginning as they gain more electrons in an attempt to gain a noble gas configuration. New shells are not formed but unpaired electrons in orbitals are now being filled. The repulsion effect is increased between shells increasing the overall atomic radius
What is the order of method of mass spectrometry?
1.Vaporisation
2.Ionisation
3.Acceleration
4.Deflection
5.Detection
Define Relative Atomic Mass
The average mass of an atom of an element compared to 1/12 of the mass of a carbon-12 isotope
Define Relative Isotopic Mass
the mass of one atom of an isotope relative to 1/12th of the mass of an atom of the isotope carbon-12
Lone pairs
a pair of valence electrons that are not shared with another atom in a covalent bond
Dative covalent bond
a covalent bond between 2 atoms where one of the atoms provides both electrons that form the bond
Order of the pairs that cause the biggest bond angle reduction
Lone pair-lone pair>lone pair-bonding pair>bonding pair- bonding pair
What is the electron pair repulsion theory?
The shape of a molecule is determined by the number of electron pairs (only valance shell) surrounding the central atom. This is because the pairs of electrons repel all the other electron pairs. The electron pairs more away from each other to achieve the maximum separation and minimum separation
Electronegativity
the ability of an atom to attract the bonding electrons towards oneself in a covalent bond
Explain the periodicity of electronegativity across periods
The electronegativity increases across periods due the shielding affect being constant and the overall nuclear charge of the nucleus attracting in the electron pair
Explain the periodicity of electronegativity down a group
The electronegativity decreases down a group as the number of electron shells increases which increases repulsion between orbitals. This increases the atomic radius and weakening the attraction between the nucleus and outermost electron and making it easier for the other electron to attract the bonding pair
Describe metallic bonding
this type of bonding is between metals where a sea of delocalised electrons flows within its structure and holds the lattice of metal cations from repelling each other as they have the same charge. this allows them to be very good conductors of electricity
What does metallic bond strength depend on?
The number of outer electrons donated to the cloud and the size of the metal cation
Explain the periodicity for boiling point in metals across periods?
The boiling point increases due to the number of electrons being donated by each metal cation to the electron cloud increasing. The increasing size of the metal ions is constant so the electron cloud becomes more effective in holding the metal cations together and stop them from repelling each other due to their same charge
How does the thermal stability of Group 1 and 2 carbonates change down a group?
Group 1 carbonates are more thermally stable as they form larger cations that have a weaker charge density compared to group 2 who form smaller cations with a stronger charge density. This means that Group 1 carbonates exert a weaker polarising force on the carbonate ion which allow it be
Why does the reactivity of Group 7 elements decrease down the group?
the distance between the nucleus and the outer electrons increases so nuclear attraction becomes weaker. This makes it harder for the atom to gain an electron and become stable.
Why does the reactivity of Group 1 elements increase down the group?
the atomic radius of the group 1 elements This means that the attraction between the nucleus and the outer electron decreases, making it easier for the atom to lose the electron.
