IB Chem flashcards

Smallest part of an element.

A substance that cannot be broken down by any chemical process into simpler substances.

The amount of substance that contains the same number of entities as there are atoms in exactly 12 grams of carbon-12.

The mass of one mole of a substance, expressed in grams per mole (g/mol).

6.022 x 10^23 mol^-1, the number of entities in one mole of a substance.

Consists of a nucleus with protons and neutrons, surrounded by electrons in orbitals.

Atom is neutral with protons = electrons; ion is charged with unequal protons and electrons.

Decreases across a period, increases down a group.

Energy to remove electrons; increases across a period, decreases down a group.

Transfer of electrons from metal to non-metal, forming positive and negative ions.

Atom's ability to attract electrons; increases across a period, decreases down a group.

Heat energy in a reaction at constant pressure.

Total enthalpy change is the same regardless of reaction steps.

Change in concentration per unit time.

Increase in temperature leads to higher reaction rate.

Rates of forward and reverse reactions are equal; concentrations remain constant.

System shifts equilibrium to counteract changes.

Measure of hydrogen ion concentration; -log[H⁺].

Strong acid fully dissociates; weak acid partially dissociates.

Oxidation is electron loss; reduction is electron gain.

Cause oxidation/reduction in other substances.

Organic compounds with the same functional group, differing by CH2.

Same formula, different atom arrangements.

Closeness to true value vs. closeness of measured values.

Fluctuations vs. consistent errors.

1s² 2s² 2p⁶ 3s².

Increases across period 3 (Na to Cl).

Increases due to added energy levels.

Sharing electron pairs between atoms.

Four covalent bonds between carbon and hydrogen.

Enthalpy change under standard conditions.

Energy absorbed = (4 × H–O) - [(2 × H–H) + (1 × O=O)].

Relationship between reaction rate and reactant concentrations.

Increases rate by providing lower activation energy pathway.

Rates of forward and reverse reactions are equal; concentrations remain constant.

Favors side with fewer gas moles.

Substances related by proton loss or gain.

pH = -log(0.10) = 1.0.

5Fe²⁺ + MnO₄⁻ + 8H⁺ → 5Fe³⁺ + Mn²⁺ + 4H₂O.

Cl₂ is oxidizing agent; Fe is reducing agent.

Group of atoms responsible for molecule's characteristic reactions.

Isobutane (2-methylpropane).

a substance that cannot be broken down into simpler substances.

smallest part of an element.

substance that contains more than one element.

this shows the simplest whole number ratio of atoms of each element in a particle of the substance.

shows the actual number of atoms of each element in a molecule of the substance.

this shows the arrangement of atoms an dbonds within a molecule.

the mass of one mole of any substance.

the weighted mean of all the naturally occurring isotopes of the elemtn relative to carbon-12

the amount of solute (dissolved substance) in a known volume of solution (solute plus solvent).

a solution of known concentration.

a gas that obeys the gas laws

a gas that hase some attractive force between the particles and do occupy some space so they do not exactly obey the gas laws.

all the collective protons and neutrons

equal to the number of protons and neutrons in the nucleus of an atom

equal to the number of protons in the nucleus and to the number of electrons in the atom

atoms of the same element with the same number of protons but with different number of neutrons

vaporized sample is injected, ionized by being bombarded with a beam of electrons until one electron is shoved off, accelerated through parallel plates where the ion is under the influence of an electric field, deflected by a magnetic field depending on mass and charge, and detected.

isotopes of elements whose nuclei break down spontaneously. they are used in nuclear power generation, the sterilization of surgical instruments, crime detection, finding cracks in metals, and food preservation.

each element has its own characteristic spectrum that is not continuous

the energy required to remove one electron from an atom in its gaseous state

the arrangement of electrons in an atom

the electrons in the highest energy level

vertical columns in the periodic table that holds elements with the same number of valence electrons

horizontal rows in the periodic table that holds elements with the same number of occupied energy shells

the distance from the nucleus to the outermost electron

positive ion. contain fewer electrons than protons so the electrostatic attraction between the nucleus and the outermost electron is greater and ion is smaller than the parent atom.

negative ion. contain more electrons than protons so it is larger than the parent atom.

the repeating pattern of physical and chemical properties shown by the different periods.

molecule with a single atom

a relative measure of the attraction an atom has for a shared pair of electrons when it is covalently bonded to another atom

an element that possesses some of the properties of a metal and some of a non-metal

substance that can be either acidic of basic.

when electrons are transferred from one atom to another to form ions with complete outer shells of elections.

involves the sharing of one or more pairs of electrons so that each atom in the molecule achieves an inert gas configuration.

it is the electron dot structure in which all the valence electrons are shown

when their is an unequal distribution of charge in a molecule

this states that pairs of electrons arrange themselves around the central atom so that they are as far apart from eachother as possible

forces that are created when an instantaneous dipole induces another dipole in a neighboring particle resutling in a weak attraction between the two particles

the attraction that two neighboring positive ions have for the delocalized electrons between them

when the heat is given out to the surroundings; the bonds in the products are stronger than the bonds in the reactants

heat is absorbed; bonds in the reactants are stronger than the bonds in the products

a measure of the total energy in a given amount of substance

a measure of the average kinetic energy of the substance

the internal energy stored in the reactants

can only be measured if products and reactants are in a gaseous state.

enthalpy change for a reaction depends only on the difference between the enthalpy of the products and the enthalpy of the reactants.

the increase or decrease in concentration of one of the products per unit time

for a reaction to occur, the particles must collide, they must collide with the proper orientation, and they must collide with enough force to bring about the reaction.

the minimum amount of energy required for a reaction to occur

when the rate of the forward reaction is equal to the rate of the reverse reaction, and both reactions continue to take place

a system in which neither matter nor energy can be lost or gained

if a system at equilibrium is subjected to a small change the equilibrium tends to shift so as to minimize the effect of the change

a substance which produces hydrogen ions

a substance than can neutralize an acid

substance that donates a proton

susbtance that accepts a proton

substance that donates a pair of electrons

substance that accepts a pair of electrons