Summer HW Vocav

Question 1

Reflux

Answer 1

A lab technique where you heat a chemical reaction mixture for a while. While heating, a condenser cools the vapor that forms, turning it back into liquid and returning it to the container. This method is useful in reactions like when you turn a primary alcohol into a carboxylic acid by oxidation

Question 2

Distillation

Answer 2

This is a method used to separate two liquids that are mixed together. The liquids must have different boiling points. During this process, the mixture is heated. The liquid with the lower boiling point evaporates first. This gas is then cooled down so it turns back into a liquid and can be collected separately from the other liquid

Question 3

Nucleon

Answer 3

particle found in the nucleus of an atom; both protons and neutrons are this

Question 4

Isotope

Answer 4

a variation of an atom from the same element, where the only difference is the number of neutrons in the nucleus. All _____ of an element have the same number of protons but different neutron counts

Question 5

Mass number

Answer 5

the total count of protons and neutrons found in the nucleus of an atom

Question 6

Relative atomic mass

Answer 6

average weight of an element’s atoms compared to a tiny fraction of a carbon-12 atom’s mass

Question 7

Atomic number

Answer 7

the number of protons in the nucleus of an atom

Question 8

Fragmentation

Answer 8

the arrangement of pieces of a molecule that you see in the results from a mass spectrometer

Question 9

Molecular ion

Answer 9

a positively charged ion produced in a mass spectrometer

Question 10

Emission spectra

Answer 10

the specific wavelengths (or colors) of light that are emitted by atoms or molecules when their electrons move from a higher energy level to a lower energy level

Question 11

Discrete

Answer 11

information that can only take certain specific values and not any value in between

Question 12

Continuous

Answer 12

information that can take any value within a range and isn’t limited to specific points

Question 13

Aufbau principle

Answer 13

a scientific principle that states that electrons will occupy the lowest energy levels of an atom before moving to higher ones

Question 14

Hund’s rule

Answer 14

a scientific principle that states that electrons fill degenerate orbitals alone before doubling up

Question 15

Pauli exclusion principle

Answer 15

a scientific principle that states that no two electrons can have exactly the same configuration. Each sub-level can hold two electrons with opposite spins

Question 16

Heisenberg uncertainty principle

Answer 16

a scientific principle that states we cannot know both the exact location and speed of an electron at the same time

Question 17

Ionization energy

Answer 17

the energy required to remove one mole of gaseous atoms to form one mole of gaseous 1+ ions

Question 18

First ionization energy

Answer 18

the energy required to remove one mole of the most loosely held electrons from one mole of gaseous atoms in the ground state

Question 19

Successive ionisation energies

Answer 19

the energies required to remove more and more electrons from an ion that is becoming increasingly positive

Question 20

Line spectrum

Answer 20

the range of frequencies or wavelengths of electromagnetic radiation emitted during an electron transition from a higher to a lower energy level

Question 21

Continuous spectrum

Answer 21

a spectrum that contains all the frequencies (or wavelengths) across a range of electromagnetic radiation.

Question 22

Convergence limit

Answer 22

the point at which the spectral lines converge. Can be used to calculate the ionization energy

Question 23

Planck’s constant

Answer 23

represented by the symbol h; helps scientists understand the relationship between energy and frequency for particles like photons

Question 24

Molecular formula

Answer 24

a type of formula that shows the actual number of atoms of each element in a molecule. (eg. butene; C4H8)

Question 24

Empirical formula

Answer 24

the simplest whole number ratio of atoms of each element in a substance. (eg. butene; CH2)

Question 24

Avogadro's constant

Answer 24

the number of particles in one mole of substance. Equal to 6.02 × 10^23

Question 25

Standard solution

Answer 25

a solution of known concentration

Question 26

Theoretical yield

Answer 26

the maximum amount of product that could be obtained from a chemical reaction, assuming all reactants are completely converted into products

Question 27

Percent yield

Answer 27

tells us how much of a product we actually make compared to how much we expected to make

Question 28

Limiting reagent/ reactant

Answer 28

the substance which is completely consumed in a chemical reaction and determines the yield of the product formed

Question 29

Atom economy

Answer 29

tells us how efficiently a reaction uses the starting materials to make the desired products

Question 30

Avogadro's law

Answer 30

equal volumes of gases at the same temperature and pressure will contain the same number of gas particles

Question 31

Ideal gas

Answer 31

are assumed to consist of particles that have negligible volume and negligible attractive forces (PV=nRT)

Question 32

Molar volume

Answer 32

tells us how much room a specific amount of gas needs when it's in its standard conditions

Question 33

Ionic bond

Answer 33

electrostatic attraction between oppositely charged ions that holds the ions in close proximity

Question 33

Electron affinity

Answer 33

the amount of energy released when a neutral atom gains an electron to form a negatively charged ion

Question 34

Covalent bond

Answer 34

the electrostatic force of attraction between two positive nuclei and a shared pair of electrons

Question 35

Bond strength

Answer 35

the amount of energy required to break a bond

Question 36

Electronegativity

Answer 36

a measure of how much an atomic nucleus attracts the shared electrons that are involved in a covalent bond

Question 37

Polarity

Answer 37

the separation of electric charge in a molecule or its chemical groups, resulting in a positive and negative end

Question 38

Electron domain

Answer 38

the region in which bonding and non-bonding pairs of electrons are most likely to be found. Non-bonding pairs, single bonds, double bonds and triple bonds each count as one electron domain

Question 39

VSEPR

Answer 39

Valence Shell Electron Pair Repulsion theory: A theory used to explain and predict molecular geometry, based on number of electron domains (bonded and non-bonded electron pairs)

Question 40

Allotrope

Answer 40

alternative forms of an elemental substance. For example, diamond and graphite are allotropes of carbon

Question 41

London dispersion force

Answer 41

the temporary instantaneous dipole formed due to the rapid and random motion of electrons

Question 42

Induced dipole moment

Answer 42

a weak intermolecular force that occurs when a polar molecule gets close to an atom or non-polar molecule and induces a dipole by disrupting the arrangement of its electrons

Question 43

Dipole-dipole interaction

Answer 43

a intermolecular force between two polar molecules that have permanent dipoles. Attractive forces exist between the positive end of one polar molecule and the negative end of another polar molecule

Question 44

Hydrogen bonding

Answer 44

the intermolecular attraction between two molecules which both contain a hydrogen bonded to a highly electronegative element such as oxygen, fluorine or nitrogen

Question 45

Delocalized electron

Answer 45

an electron that is not associated with one specific atom and is free to move within the molecular structure

Question 46

Alloy

Answer 46

homogeneous mixtures of a metal and other metals or non-metals

Question 47

Atomic radius

Answer 47

the distance from an atom's nucleus to the outermost orbital of one of its electrons. Usually measured as the half-distance between the nuclei of two of the same atoms bonded together

Question 48

Ionic radius

Answer 48

the distance between the nucleus of an ion and the outermost shell of the ion

Question 49

Isoelectronic

Answer 49

molecules with the same electron configuration

Question 50

Oxidation state/number

Answer 50

a number assigned to an element showing the number of electrons lost or gained (or even shared) in a compound or ion

Question 51

Homologous series

Answer 51

a series of organic compounds with the same functional group that differ by a common structural unit

Question 52

Structural isomer

Answer 52

compounds with the same molecular formula but different structural arrangements

Question 53

Skeletal formula

Answer 53

a type of formula that only shows the carbon skeleton (or backbone) of an organic compound

Question 54

Functional group

Answer 54

group of atoms present on a molecule that give physical and chemical properties to a compound

Question 55

Enthalpy

Answer 55

measurement of heat energy within a system. It is symbolised in expressions by H

Question 56

Specific heat capacity

Answer 56

the quantity of heat needed to raise the temperature per unit mass

Question 57

Standard enthalpy of reaction

Answer 57

the heat energy transferred within a reaction under standard conditions with all substances present in their standard states

Question 58

Average bond enthalpy

Answer 58

the enthalpy change when one mole of bonds are broken in the gaseous state averaged for the same bond in similar compounds

Question 59

Hess's law

Answer 59

law that states that the total enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place, as long as the initial and final conditions are the same

Question 60

Equilibrium constant

Answer 60

ratio between the concentration of products and reactants for a reversible reaction at equilibrium

Question 61

Collision theory

Answer 61

an explanation of how reactions take place, which states that for reactions to happen the particles must collide with a minimum amount of energy and the collisions must have the correct collision geometry

Question 62

Catalyst

Answer 62

a substance that changes the rate of a reaction and is not used up. Although it speeds up a reaction, the catalyst itself is not changed by the reaction. Negative catalysts also exist - substances that slow down the rate of a reaction

Question 63

Dynamic equilibrium

Answer 63

a state in chemistry that occurs when a reversible reaction happens in a closed container at the same rate in both directions. This means that the reactants and products are constantly transitioning between each other at equal rates, resulting in no net change and no observable change in the system's properties

Question 64

Le Chatelier's Principle

Answer 64

a principle used to predict in which direction the equilibrium position will shift when changes are made to a reaction at equilibrium

Question 65

Equilibrium law

Answer 65

the principle that (at chemical equilibrium) in a reversible reaction the ratio of the rate of the forward reaction to the rate of the reverse reaction is a constant for that reaction