Energy levels are closer together at high energy levels.
First ionization energy. The convergence limit is an electron moving from the lowest energy level to the highest one which is equal to the energy required to move the first electron from a gaseous atom.
Electrons in discrete energy levels Energy levels get closer together at higher energy levels
The emission spectrum of hydrogen contains only certain frequencies instead of continuous frequencies and those frequencies converge at higher frequencies.
Electrons transfer between higher energy levels to lower energy levels.
Electron transitions into first energy level causes UV series
Electron transitions into second energy level causes visible series
Electron transitions into third energy level causes infrared series
The Ionic radius of nitrogen is greater than the atomic radius due to increased repulsion between electrons.
A metal that has stable ions that contain the incomplete d shells.
Water donates a lone electron pair to vanadium ions through the formation of a dative covalent bond.
The absorption of wavelengths will increase because Chloride ions are a weaker ligand than water, so there is a smaller energy gap between split d-orbitals.
Two O atoms of the ethanedioate ions can provide two electron pairs to form two coordinate bonds with the metal ion.
The oxides of period 3 are changed from basic to acidic through amphoteric.
Transition metals contain the partially filled d-orbitals. When ligands bind into the transition metal, it causes d-d splitting. When electrons transit to a higher energy level, visible Light which is equal to the energy difference is absorbed. The color observed is the complementary color.
Transition metals contain the partially filled d-orbitals. Color depends upon the energy difference between the split d-orbitals. The split d-orbitals depend on variable oxidation states, different ligands, and different numbers of ligands.
Across period 3, all atoms have the same number of occupied electron shells and similar shielding effects. However, there is an increasing number of protons causing the increase in effective nuclear charge. Therefore, the attraction between the nucleus and outer shell electrons increases and creates the energy needed to remove the first electron from the atoms.
P4O10 (s) + 6 H2O —-> 4 H3PO4
Molecules have more than one possible position for the multiple bonds.
In the dinitrogen monoxide molecules, sigma bonds from N to N and from N to O while Pi bonds from N to N. Delocalized pi bond extends over the oxygen and both nitrogens.
Giant lattice structures and electrostatic attraction between Magnesium ions and oxide ions.
Electrostatic attraction between a lattice of metal ions and delocalized electrons.
Vanadium has a smaller ionic radius than titanium leading to stronger metallic bonding. Therefore, more energy is required to break the metallic bond in vanadium.
Titanium atoms are of different sizes to aluminum atoms to prevent layers from sliding over each other.
In ozone, a lone pair of p orbital of the O atom overlaps with pi electrons from a double bond. Therefore, both O-O bonds have equal bond length and equal bond energy.
Oxygen is an element in the standard conditions.
Tin(II) ion has the same charger as well as a similar ionic radius to the Strontium ion.
Ethanoic acid is weak acid while hydrochloric acid is strong acid. Energy is used to ionize weak acids before a reaction with NaOH can occur.
The frequency(pre-exponential) factor, A, is indicative of the frequency of collisions and the probability that collisions have proper orientations.
Increasing the temperature will increase the kinetic energy, particles move fast and have high collision frequency. Also, a greater proportion of molecules have energy greater than the activation energy. Greater successful collision frequency.
At higher temperatures, rates of reactions are faster, shorten reaction time so larger percentage error in timing.
Increasing the concentration will increase the number of particles per unit volume, particles have higher collision frequency to cause greater successful collision frequency.
Decreasing the particle size will increase the total surface area, particles have more right orientation to collide and cause greater successful collision frequency.
Decreasing the particle size will increase the total surface area, particles have more right orientation to collide and cause greater successful collision frequency.
Catalysts will alternate reaction pathways with lower activation energy. This causes a greater proportion of molecules to have energy greater than the activation energy. Greater successful collision frequency.
Dynamic equilibrium is established when the rate of forward reaction equals rate of reverse reaction. As a result, the concentrations of reactants and products become and remain constant.
If a system at equilibrium is disturbed by a change in temperature, pressure, or the concentration of one the components, the system will shift its equilibrium position so as to oppose the effect of the change.
With an increase in [reactant], the equilibrium shifts to the right to decrease the [reactant] and to increase [products].
Increasing temperature will shift the equilibrium position to the endothermic side to decrease the temperature.
Catalysts do not affect the position of an equilibrium as catalysts speed up the rates of both forward and reverse reactions equally!
A species partially dissociates the proton ion.
A species can act as both a bronsted-lowry acid and a bronsted-lowry base.
Phosphorus is not commonly found in fuels and phosphorus oxides are solids that are not easily distributed in the atmosphere.
Species that have one less proton than its conjugate acid.
It will produce chlorine gas in reaction with ClO- which is toxic
In the conversion of P4 to H2PO2-, oxygen is gained,so can be oxidation while hydrogen gained, so can be reduced. The two definitions led to conflicting results.
Using inert Pt as an electrode and 1 mol dm-3 H+ as electrolyte and bubbling Hydrogen gas into the solution under 100 kpa.
X-ray crystallography shows that benzene is of hexagon planar shape and C to C bond lengths are all equal and C-C-C bond angles are all equal.
It is the minimum energy required to remove an electron from a neutral gaseous atom or molecule in its ground state.
All collisions are perfectly elastic (which means no energy is lost during collision.)
No intermolecular forces between gas molecules
The volume occupied by individual gas molecules is negligible
In benzene, electrons are delocalized between the six carbons while π-electrons are localized between two carbons in alkenes. Therefore, benzene has a lower electron density than alkene and induces a weaker dipole in the attacking molecule.
A sigma bond is formed by the head-on combination of the atomic orbitals where the electron density is concentrated along the bond axis. A Pi bond is formed by the lateral combination of p-orbitals whether electron density is concentrated on opposite sides of the bond axis
Hybridization is a term used to describe the mixing of atomic orbitals to generate a set of new hybrid orbitals that are equivalent.
It is an ion or molecule which can donate its lone pair electron to the metal ion center forming a dative covalent bond
It is the relative measure of an atom to attract a bonding pair of electrons in a covalent bond.
Organic compounds in a homologous series have similar chemical properties.
All members have the same suffix.
The successive members of a homologous series differ by a unit of CH2
The physical properties of a homologous series show a trend.
Structural isomers are molecules that have the same molecular formula but different connectivities.
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