General Chemistry Flashcards
He discovered the nucleus with his “Gold Foil” experiment.
Ernest Rutherford
He is credited with the discovery of electron in an atom.
J.J. Thomson
Which of the following is an intensive property?
Density
Which of the following is an extensive property?
Weight
Brass is an example of ___________.
Homogeneous mixture
Methane is an example of __________.
Compound
Which of the following is not an example of observable physical
property?
Mass
It is the number of proton in nucleus.
Atomic number
Atoms of the same element with varying number of neutrons
Isotopes
He formulated the Periodic Law.
Dmitri Mendeleev
He arranged the elements in the periodic table in groups of 8’s like
from lithium to sodium also known as “Law of Octaves”.
John Newlands
He arranged the elements in the periodic table in groups of 3’s or
triads also known as “Law of Triad”.
Johann Wolfgang Dobereiner
A substance that has the ability to dissolve or disperse one or more substances?
Solvent
A solution with solute that dissolves until it is unable to dissolve anymore, leaving the undissolved substances at the bottom.
Saturated solution
A solution that completely dissolves, leaving no remaining
substances.
Unsaturated solution
A solution that contains more undissolved solute than the saturated solution because of its tendency to crystallize and precipitate.
Supersaturated solution
Which of the following is arranged in increasing atomic size?
Mg > Ca > K > Fr
Which of the following elements is more electronegative: Cl, S, or
Mg?
Cl
Which of the following elements is more reactive: Li, Rb, or Fr?
Fr
The seven horizontal rows in the periodic table are called __________.
Periods
Group 7A is a family of _______
Halogens
It is the most ideal gas element.
Helium
These are properties that determine whether or not a substance will react chemically.
Chemical Properties (flammability, reactivity)
Which of the following elements (Br or Cu) has the higher ionization energy?
Br
Which has a larger ionic size ( Na+ or Mg2+)
Na+
Sodium carbonate is also known as?
Soda ash
Agua regia is a/an ______.
solution
It does not depend on the size or amount of the sample.
Intensive Property (color, odor, boiling point)
These are properties that can be observed or measured.
Physical Properties (color, mass, length, volume, density, state,
conductivity, temperature.)
Possible indication of chemical change:
- Change in color
- Change in temperature
- Apperance or disappearance of precipitate
- Evolution of gas
Each element is
composed of extremely small particles called atoms.
Dalton’s Billiard Ball Model (1803)
The atom is made up of negative electrons that float in a sphere of
positive charge like plums in a pudding. He discovered electron (cathode ray experiment).
Thomson’s Plum Pudding Model (1904)
Discovered the nucleus of a gold atom with his “gold foil” experiment.
Rutherford’s Nuclear Model (1911)
It depends on the size or amount of the sample.
Extensive Property (mass, volume)
Nucleus surrounded by
orbiting electrons at different energy levels.
Bohr’s Planetary Model (1913)
He formulated the Periodic Law.
Dmitri Mendeleev
“Law of Octaves”
John Newlands
He recognized the repeating pattern or the periodic behavior among elements. He studied the
relationship of the atomic volume and the relative atomic mass of 28 elements.
Julius Lothar Meyer
It is the average distance between
nucleus and the valence electron.
Atomic Size (Atomic Radius)
“Law of Triad”
Johann Wolfgang Dobereiner
It is the ability of the atom to donate electrons.
Metallic Property
Cation Radius < Neutral Atomic Radius (Example: Al3+ < Al )
Anion Radius > Neutral Atomic Radius (Example: O2− > O )
It is the change in energy when an electron is accepted by a gaseous atom to form an anion.
Electron Affinity
It is tendency of an atom to react.
Reactivity
It is defined as the relative ability of an atom of an element to attract or gain electrons.
Electronegativity
Decreasing (top to bottom, right to left)
Ionization energy, electron affinity, electronegativity
It is the amount of energy required to remove an electron from an atom or ion.
Ionization Energy
Increasing (top to bottom, right to left)
Atomic size, metallic property, reactivity
It tells the shape of the orbital.
Azimuthal / Angular Momentum Quantum Number (l)
The average distance of the electron from the nucleus in a particular orbital.
Principal Quantum Number (n)
It describes the orientation of orbital.
Magnetic Quantum Number (ml)
It shows the spin of electrons.
Spin Quantum Number (ms)
Electron-transfer where one of the reacting atoms loses one or more electrons and the other atom gains
on or more electrons. (metal to non-metal)
Ionic Bonding
It is formed by electron sharing,
usually between atoms of non-metals. (non-metal to non-metal).
Covalent Bonding
The ratio of the total mass of each element to the total mass of one mole of the compound (MM) multiplied by 100%.
Percent Composition
Gives the actual ratio of the number of moles of atoms in a mole of the compound.
Molecular Formula
A mole is the amount of substance
that contains Avogadro’s number of particles equal to 6.02x1023.
Avogadro’s number
Ability of a solvent to dissolve a salt at a particular temperature.
Solubility
Solvent can still dissolve the
solute.
Unsaturated Solution
Gives the simplest ratio of the
number of moles of atoms.
Empirical Formula
If a solvent can’t no longer
dissolve a given solute at a given temperature.
Saturated Solution
It is the sum of the atomic
masses (in u) of all the atoms in a molecule.
Molecular Mass (amu)
It is the mass in grams of one mole
of a substance.
Molar Mass (g/mol)
If the solvent can’t dissolve
the solute and need to be heated for it to be dissolved.
Supersaturated Solution
