Q1 Flashcards
Study of matter, its characteristics, composition, and transformation.
CHEMISTRY
anything that occupies space and has mass.
Matter
the amount of matter.
Mass
mass dependent on gravity; acceleration due to gravity.
Weight
is the measure of the amount of occupied space.
Volume
State of matter that has a definite shape and definite volume.
Solid
State of matter that has indefinite shape (it takes the shape of its container), and a definite volume.
Liquid
State of matter that has indefinite shape and indefinite volume (assumes the shape and volume of its container).
Gas
What is the particle motion of solid matter?
intact; vibrates only due to its compactness
What is the particle motion of liquid matter?
has space; particles flows through each other
What is the particle motion of gas matter?
particles are apart from each other; moves fast
ratio of the mass of an object to the volume occupied by that object.
Density
is a measure of the change in volume of a sample of matter resulting from a pressure change.
Compressibility
is a measure of the change in volume of a sample of matter resulting from a temperature change.
Thermal expansion
illustrates the composition of matter
Space filling model
distinguishing characteristic that is used in the identification and description of matter
Property of matter
observable characteristics without changing composition (ex: color and shape; solid, liquid, or gas; boiling point, melting point)
Physical property
not dependent on mass (ex: boiling point, color, temperature, luster, hardness).
Intensive properties
Intensive or extensive: Boiling point
Intensive
Intensive or extensive: Color
Intensive
Intensive or extensive: Temperature
Intensive
Intensive or extensive: Luster
Intensive
Intensive or extensive: Hardness
Intensive
Intensive or extensive: Volume
Extensive
Intensive or extensive: Mass
Extensive
Intensive or extensive: Size
Extensive
Intensive or extensive: Length
Extensive
changes observable without changing composition (ex; changes in physical state: melting, boiling, freezing; change in state of subdivision with no change in physical state (ex: pulverizing a solid).
PHYSICAL CHANGE
chemical identity; properties that describe how a substance changes (or resists change) to form a new substance
Chemical property
changes in which one or more new substances are formed (ex: decomposition, reaction with another substance).
Chemical change
Physical or chemical property: Boiling point
Physical
Physical or chemical property: Phase (solid, liquid, gas)
Physical
Physical or chemical property: Color
Physical
Physical or chemical property: Flammability
Chemical
Physical or chemical property: Decomposition
Chemical
a single kind of matter that cannot be separated into other kinds of matter by physical means. always has a definite and constant composition and has the same properties under the same condition.
Pure Substances
a pure substance that is composed of only one kind of atom. Cannot be broken down into simpler substances by chemical or physical means.
Element
a pure substance that is composed of two or more different kinds of atoms. Can be broken down into constituent elements by chemical, but not physical means.
Compound
Physical combination of 2 or more substances; each substance retains its chemical identity. Can be physically mixed, physically separated.
Mixtures
Contains only one visible distinct part (phase) which has uniform properties throughout. The components cannot be visually distinguished.
Homogenous Mixture
Contains visibly different distinct parts (phases), each of which has different properties. A nonuniform appearance is a characteristic of this type.
Heterogenous Mixture
have particles bigger than of a solution but smaller than of suspension. Particles are distributed throughout the mixture without settling.
Colloids or colloidal dispersion
have particles bigger than of colloids which eventually settle after interacting with a solvent-like phase. (ex: mud & mustard)
Suspensions
Who is the proponent of the Atomic Theory?
John Dalton
Atomic theory #1
Each element is composed of extremely small particles called atoms.
Atomic theory #2
All atoms of a given element are identical, but the atoms of one element are different from the atoms of all other elements.
Atomic theory #3
Atoms of one elements, cannot be changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions.
Atomic theory #4
Compounds are formed when atoms of more than one elements combine; a given compound always has the same relative number and kind of atoms.
Revision #1
Atoms are not indestructible.
Revision #2
The atoms of one element may differ in mass.
States that compounds have a definite composition regardless of how the samples were prepared or where they originated.
LAW OF DEFINITE PROPORTION
States that during physical and chemical change, the total mass of all substances before and after the change are the same. Atoms are either created nor destroyed.
LAW OF CONSERVATION OF MASS
States that if two elements A and B combine to form more than one compound, the masses of B that can combine with a given mass of A are in the ration of small whole numbers.
LAW OF MULTIPLE PROPORTION
Are building blocks of matter and are the smallest particles of an element that retain the chemical identity of the element.
Atoms
the building blocks for atoms.
Subatomic particles
the lightest Subatomic particle
Electrons
Possesses a positive electrical charge
Protons
Has no charge, it is neutral.
Neutrons
Contains the nucleons (protons and neutrons).
Nucleus
Is where the electrons move rapidly about the nucleus.
EXTRANUCLEAR REGION
Denoted by (Z). The number of protons and electrons.
Atomic number
Is the sum of protons and neutrons in the nucleus of an atom.
MASS NUMBER
Is a notation where the atomic number is placed as a subscript and the mass number is placed as a superscript in front of the chemical symbol.
COMPLETE CHEMICAL SYMBOL NOTATION
atoms of an element that have different numbers of neutrons. The same atomic number but different mass numbers.
Isotopes
emit radiation spontaneously and these are used for diagnostic and therapeutic purposes.
Radioactive Isotopes
Is a group of two or more atoms that functions as a unit and capable of stable independent existence.
Molecules
Contains atoms that are of the same kind. This molecule must be an element.
Homoatomic molecules
Contains two or more kinds of atoms. This molecule must be a compound.
Heteroatomic Molecule
an atom or a group of atoms that has a net positive charge or a negative charge.
Ions
tend to lose electrons to form cations
Metals
tend to gain electrons to form anions.
Non metals
Is used to express the composition of molecules and ionic compounds in terms of chemical symbols.
CHEMICAL FORMULA
Is a representation of a compound’s structure in a 3-dimensional molecular view.
MOLECULAR MODELS
Shows exact numbers of atoms of each elements
Molecular formula
Shows number of atoms in the simplest whole number ratio of atoms present
Empirical formula
Indicates arrangement and bonds; graphical representations
Structural formula
Model by John Dalton
Soldi Sphere Model
Who first proposed the idea of the indivisible particle ‘atomos’?
Democritus
His theory stated that atoms are indivisible, those of a given element are identical, and compounds are combinations of different types of atoms.
John Dalton’s Solid Sphere Model
Model by JJ Thomson
Plum Pudding Model
It shows the atom as composed of electrons scattered throughout a spherical cloud of positive charge.
JJ Thomson’s Plum Pudding Model
Model by Ernest Rutherford
Nuclear Model
Father of Nuclear Age; conducted the gold foil experiment
Ernest Rutherford
Discovery of the positive charged concentrate part called nucleus.
Ernest Rutherford’s Nuclear Model
Model by Niels Bohr
Planetary Model
stating that electrons moved around the nucleus in orbits of fixed sizes and energies. Electron energy in this model was quantised; electrons could not occupy the values of energy between the fixed energy levels.
Niels Bohr’s Planetary Model
Model by Erwin Schrodinger
Quantum Model
electrons do not move in set paths around the nucleus, but in waves. It is impossible to know the exact location of the electrons; instead, we have ‘clouds of probability’ called orbitals, in which we are more likely to find an electron.
Erwin Schrodiner’s Quantum Model
Is a region of space about a nucleus that contains electrons that have approximately the same energy and that spend most of their time approximately the same distance from the nucleus.
Energy Level or Shell
region of space within the energy level (shell) that contains electrons that have the same energy.
Sublevel or subshell
Is a region of space within the subshell (sublevel) where an electron with a specific energy is not most likely to be found.
Orbital
Are the orbitals in the same subshell (sublevel) which have the same energy (e.g. the three 2- orbitals in the 2- subshell)
DEGENERATE ORBITALS
required to describe the distribution of electrons
Quantum numbers
refers to the main energy level of an orbital and can have integral values from 1, 2, 3 and so forth.
PRINCIPAL QUANTUM NUMBER (n)
Represent energy sublevels (subshells) and tells us the shape of the orbitals. For given value of n, l has possible integral values from 0 to (n - 1)
ANGULAR MOMENTUM QUANTUM NUMBER (l)
Determines the orientation of the orbitals within a subshell
Magnetic Quantum Number (ml)
Determines the spin/direction of the arrow
Spin Quantum Number (ms)
How many electrons an atom has in each of its electron subshells
Electron configuration
states that the electron subshells are filled in order of increasing energy.
Aufbau Principle
states that electrons occupy the orbitals of a subshell (degenerate orbitals) such that each orbital acquires a second electron. All electrons in such singly occupied orbitals must have the same spin.
HUND’S RULE
no two electrons in the same atom can have the same set of quantum numbers. No more than two electrons may exist in a given orbital– and then only if they have opposite spins.
PAULI EXCLUSION PRINCIPLE
Is a notation that shows how many electrons an atom has in each of its occupied orbitals
Orbital diagrams
A rectangular box contains the symbol, atomic number and atomic mass of the element.
Periodic Table
Arrangement of the elements in the periodic table
Increasing atomic number
Is a horizontal row of elements in the periodic table which are numbered sequentially with Arabic numbers.
Period
Is a vertical column in the periodic table. There are two notations for designating the group of elements.
Group
Are elements which have the properties of both metals and nonmetals.
Metalloids
Have a distinguishing electron that completes the p subshell (except He with 1s2 ).
NOBLE-GAS ELEMENTS
Have the distinguishing electron partially or completely fill the s and p subshell.
REPRESENTATIVE ELEMENTS
Have the distinguishing electron in the d subshell.
TRANSITION ELEMENTS
Have distinguishing electron in an f subshell.
INNER TRANSITION ELEMENTS
States that when elements are arranged in order of increasing atomic number, elements with similar chemical properties occur at periodic intervals.
PERIODIC LAW
Is the nuclear charge felt by an electron when both the actual nuclear charge (Z) and the repulsive effects (shielding) of the other electrons are taken into account.
EFFECTIVE NUCLEAR CHARGE (Zeff)
is the minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion.
IONIZATION ENERGY
the energy needed to remove the first electron from a neutral atom
first ionization energy
the energy needed to removed the second electron, and so forth.
second ionization energy
Is the energy change that occurs when an electron is added to a gaseous atom to form negatively charged ions. This measures the ease with which an atom gains an electron. The ability to accept one or more elements also greatly influences the chemical behavior of atoms.
ELECTRON AFFINITY
