AP Chem Ch2 Flashcards
According to Barron’s, what is the bottom number in the Periodic Table cell?
Atomic mass, not Atomic weight.
Sodium Symbol
Na
Potassium Symbol
K
Iron Symbol
Fe
Silver Symbol
Ag
Tin Symbol
Sn
Antimony Symbol
Sb
Tungsten Symbol
W
Gold Symbol
Au
Mercury Symbol
Hg
Lead symbol
Pb
(W.r.t. element symbol scripts). Upper left
Mass number (mass of an isotope aka isotope mass), A
(W.r.t. element symbol scripts). Lower left
Atomic number, Z
(W.r.t. element symbol scripts). Upper right
charge
(W.r.t. element symbol scripts). Bottom right
How many atoms of the given element are present
Radio-isotope
An isotope that has an unstable nucleus and is therefore radioactive.
Radioactive
W.r.t. atoms, a nucleus whose constituents are unstable and emitting (radiating) particles.
Subatomic particles that are radiated
Beta (electron when negative, positron when positive), neutron, helium nucleus (alpha particle).
Nuclear mass
Atomic mass A.
Nuclear charge
Atomic number Z.
What does radiation cause to happen with the nucleus?
Change from one isotope to another
What type of energy is released with nuclear radiation?
X-rays or gamma rays.
Alkali metals
Group 1
Alkali earth metals
Group 2
Transition elements
Group 3-12
Halogens
Group 17
Noble gases
Group 18
Differentiating electron
The electron that makes a given element different from another.
Isoelectronic
Atoms and ions that have identical electron configurations.
2 out of all elements that are liquid under “normal” conditions.
Mercury and bromine.
Elements that are gases at room temp.
Noble gases, hydrogen, nitrogen, oxygen, fluorine, and chlorine.
Diatomic elements
H, O, N and the halogens.
allotrope
An element that exists in different forms (O2 and O3 e.g.)
Melting point trends
For metals: decreases as you go down the periodic table.
For non-metals: increase as you down the periodic table.
Atomic radii trends
Increases as you go down PT, decreases as you go right (stronger positive pull aka effective nuclear charge).
Effective nuclear charge
The net positive charge experienced by an electron in an atom. Note that core electrons shield valence electrons to some extent. However, other valence electrons do not shield other valence electrons from the remaining effective nuclear charge. The resulting trend is very counter intuitive - it is like electro-negativity EXCEPT it doesn’t vary vertically.
Ionization energy
The energy needed to remove an electron from an atom completely. It is always endothermic (energy must be added to remove the electron).
Photoelectric effect (and who discovered it)
The effect where electromagnetic radiation causes an electron to be ejected from a material. Einstein.
Binding energy equation
Binding energy = Eincoming - Eemitted
Photoelectron spectrometers
Used to measure the kinetic energies of ejected electrons during a photoelectric effect.
Electron affinity
The energy change that accompanies the addition of an electron to an atom. Can be thought of as the amount of energy needed to add an electron. The higher the harder.
Electronegativity
How readily an atom accepts another electron.
Sizes of cations vs anions
Cations are smallest (less pushing), then neutral, then the largest is anions.
