Atoms, moles and stoichiometry Flashcards
What is an anode?
The positive electrode (where oxidation occurs).
What is the relative mass of an electron?
1/1836
What is an atomic number?
The number of protons in the nucleus of an atom. Also called the proton number.
What is an isotope?
Atoms of the same element with different mass numbers.
What is the mass number?
The number of protons+neutrons in an atom. Also called the nucleon number.
Do isotopes of a particular element have similar chemical properties?
Isotopes of a particular element have the same chemical properties because they have the same number of electrons.
Do isotopes of a particular element have similar physical properties?
Isotopes of a particular element have slightly different physical properties, such as small differences in mass and density because they have a different number of neutrons.
What are two ways isotopes can be represented?
isotopes can be represented by nuclide notation. Chemists also name them by emitting the proton number and placing the nucleon number after the name for example the isotopes of hydrogen can be called:
hydrogen-1
hydrogen-2
hydrogen-3
Explain the behaviour of subatomic particles in an electrical behaviour field.
Beams of protons and electrons are deflected by electrical fields but neutrons are not.
What is electron configuration?
The arrangement of electrons in an atom is called its electronic structure or electronic configuration.
What are quantum shells?
Electrons are arranged outside the nucleus in energy levels or quantum shells. These principle energy levels or principle quantum shells (symbolled n) are numbered according to how far they are from the nucleus. The lowest energy level n=1 is closest to the nucleus, the energy level n=2 is further out and so on.
Which electrons have greater energy?
The electrons in quantum shells further away from the nucleus have more energy and are held less tightly to the nucleus.
How many maximum electrons can principle quantum shells hold?
Shell 1: 2 electrons
Shell 2: 8 electrons
Shell 3: 18 electrons
Shell 4: 32 electrons
What is the first ionization energy, IE1?
First Ionisation energy is the energy needed to remove one mole of electrons from 1 mole of atoms of an element in the gaseous state to form one mole of gaseous ions.
What is ionisations energies units?
Its units are KJ mol-1
What is successive ionisation energy?
We can continue to remove electrons from an atom until only the nucleus is left. We call this sequence of ionization energies successive ionisation energies.
What is second ionisation energy?
The second ionisation energy is the energy needed to remove 1 electron from each ion of an element in 1 mole of gaseous +1 ions to form 1 mole of gaseous ions with a +2 charge.
What is the trend in ionisation energy across a period and down a group?
The first ionisation energy increases across a period and decreases down a group.
Why does ionisation energy increase across a period?
Across a period from left to right, the ionisation energy increases as with each successive element one proton is added so the nucleus is becoming more positive. This increase in nuclear charge exerts a greater electrostatic attraction on the electrons and therefore more energy is required to remove electrons.
Why does ionisation energy decrease down a group?
Going down a group, the ionisation energy decreases. This is because with each successive element there is an extra occupied energy level so the electron being removed is further away from the nucleus. Also, this electron is more shielded from the positive charge of the nucleus, by the extra inner occupied energy levels. This increased distance and shielding of the outer electrons from the nucleus, makes the electrostatic attraction weaker and electrons are more easily removed.
What is shielding?
Shielding is the ability of inner shell electrons to reduce the effect of the nuclear charge on outer shell electrons.
What are the four factors which influence ionisation energy?
Four factors that influence ionisation energy are:
The size of the nuclear charge
Distance of Outer electrons from the nucleus
Shielding effect of inner electrons
Spin Pair repulsion
What is the general relationship between ionization energy and nuclear charge?
In general, ionisation energy increases as the proton number increases.
What is the general relationship between the distance of the outer electron shell and ionisation energy?
In general, the further the outer electron is from the nucleus, the lower the ionisation energy.
What is the general relationship between the shielding effect of inner electrons and ionisation energy?
In general ionisation energy is lower as the number of full outer electron shells between the outer electrons and the nucleus increases.
What is the general trend between spin pair repulsion and ionisation energy?
Increased repulsion makes it easier to remove an electron so ionization energy decreases.