Q1 Flashcards
(117 cards)
1
Q
Study of matter, its characteristics, composition, and transformation.
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CHEMISTRY
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Q
anything that occupies space and has mass.
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Matter
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the amount of matter.
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Mass
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mass dependent on gravity; acceleration due to gravity.
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Weight
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is the measure of the amount of occupied space.
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Volume
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State of matter that has a definite shape and definite volume.
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Solid
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State of matter that has indefinite shape (it takes the shape of its container), and a definite volume.
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Liquid
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State of matter that has indefinite shape and indefinite volume (assumes the shape and volume of its container).
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Gas
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Q
What is the particle motion of solid matter?
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intact; vibrates only due to its compactness
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Q
What is the particle motion of liquid matter?
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has space; particles flows through each other
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Q
What is the particle motion of gas matter?
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particles are apart from each other; moves fast
12
Q
ratio of the mass of an object to the volume occupied by that object.
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Density
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is a measure of the change in volume of a sample of matter resulting from a pressure change.
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Compressibility
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is a measure of the change in volume of a sample of matter resulting from a temperature change.
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Thermal expansion
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illustrates the composition of matter
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Space filling model
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distinguishing characteristic that is used in the identification and description of matter
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Property of matter
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observable characteristics without changing composition (ex: color and shape; solid, liquid, or gas; boiling point, melting point)
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Physical property
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not dependent on mass (ex: boiling point, color, temperature, luster, hardness).
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Intensive properties
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Intensive or extensive: Boiling point
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Intensive
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Intensive or extensive: Color
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Intensive
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Intensive or extensive: Temperature
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Intensive
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Intensive or extensive: Luster
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Intensive
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Intensive or extensive: Hardness
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Intensive
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Intensive or extensive: Volume
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Extensive
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Intensive or extensive: Mass
Extensive
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Intensive or extensive: Size
Extensive
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Intensive or extensive: Length
Extensive
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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
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chemical identity; properties that describe how a substance changes (or resists change) to form a new substance
Chemical property
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changes in which one or more new substances are formed (ex: decomposition, reaction with another substance).
Chemical change
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Physical or chemical property: Boiling point
Physical
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Physical or chemical property: Phase (solid, liquid, gas)
Physical
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Physical or chemical property: Color
Physical
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Physical or chemical property: Flammability
Chemical
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Physical or chemical property: Decomposition
Chemical
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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
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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
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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
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Physical combination of 2 or more substances; each substance retains its chemical identity. Can be physically mixed, physically separated.
Mixtures
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Contains only one visible distinct part (phase) which has uniform properties throughout. The components cannot be visually distinguished.
Homogenous Mixture
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Contains visibly different distinct parts (phases), each of which has different properties. A nonuniform appearance is a characteristic of this type.
Heterogenous Mixture
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have particles bigger than of a solution but smaller than of suspension. Particles are distributed throughout the mixture without settling.
Colloids or colloidal dispersion
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have particles bigger than of colloids which eventually settle after interacting with a solvent-like phase. (ex: mud & mustard)
Suspensions
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Who is the proponent of the Atomic Theory?
John Dalton
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Atomic theory #1
Each element is composed of extremely small particles called atoms.
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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.
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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.
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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.
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Revision #1
Atoms are not indestructible.
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Revision #2
The atoms of one element may differ in mass.
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States that compounds have a definite composition regardless of how the samples were prepared or where they originated.
LAW OF DEFINITE PROPORTION
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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
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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
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Are building blocks of matter and are the smallest particles of an element that retain the chemical identity of the element.
Atoms
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the building blocks for atoms.
Subatomic particles
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the lightest Subatomic particle
Electrons
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Possesses a positive electrical charge
Protons
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Has no charge, it is neutral.
Neutrons
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Contains the nucleons (protons and neutrons).
Nucleus
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Is where the electrons move rapidly about the nucleus.
EXTRANUCLEAR REGION
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Denoted by (Z). The number of protons and electrons.
Atomic number
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Is the sum of protons and neutrons in the nucleus of an atom.
MASS NUMBER
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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
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atoms of an element that have different numbers of neutrons. The same atomic number but different mass numbers.
Isotopes
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emit radiation spontaneously and these are used for diagnostic and therapeutic purposes.
Radioactive Isotopes
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Is a group of two or more atoms that functions as a unit and capable of stable independent existence.
Molecules
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Contains atoms that are of the same kind. This molecule must be an element.
Homoatomic molecules
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Contains two or more kinds of atoms. This molecule must be a compound.
Heteroatomic Molecule
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an atom or a group of atoms that has a net positive charge or a negative charge.
Ions
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tend to lose electrons to form cations
Metals
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tend to gain electrons to form anions.
Non metals
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Is used to express the composition of molecules and ionic compounds in terms of chemical symbols.
CHEMICAL FORMULA
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Is a representation of a compound’s structure in a 3-dimensional molecular view.
MOLECULAR MODELS
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Shows exact numbers of atoms of each elements
Molecular formula
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Shows number of atoms in the simplest whole number ratio of atoms present
Empirical formula
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Indicates arrangement and bonds; graphical representations
Structural formula
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Model by John Dalton
Soldi Sphere Model
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Who first proposed the idea of the indivisible particle ‘atomos’?
Democritus
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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
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Model by JJ Thomson
Plum Pudding Model
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It shows the atom as composed of electrons scattered throughout a spherical cloud of positive charge.
JJ Thomson’s Plum Pudding Model
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Model by Ernest Rutherford
Nuclear Model
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Father of Nuclear Age; conducted the gold foil experiment
Ernest Rutherford
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Discovery of the positive charged concentrate part called nucleus.
Ernest Rutherford’s Nuclear Model
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Model by Niels Bohr
Planetary Model
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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
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Model by Erwin Schrodinger
Quantum Model
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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
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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
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region of space within the energy level (shell) that contains electrons that have the same energy.
Sublevel or subshell
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Is a region of space within the subshell (sublevel) where an electron with a specific energy is not most likely to be found.
Orbital
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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
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required to describe the distribution of electrons
Quantum numbers
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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)
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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)
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Determines the orientation of the orbitals within a subshell
Magnetic Quantum Number (ml)
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Determines the spin/direction of the arrow
Spin Quantum Number (ms)
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How many electrons an atom has in each of its electron subshells
Electron configuration
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states that the electron subshells are filled in order of increasing energy.
Aufbau Principle
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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
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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
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Is a notation that shows how many electrons an atom has in each of its occupied orbitals
Orbital diagrams
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A rectangular box contains the symbol, atomic number and atomic mass of the element.
Periodic Table
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Arrangement of the elements in the periodic table
Increasing atomic number
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Is a horizontal row of elements in the periodic table which are numbered sequentially with Arabic numbers.
Period
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Is a vertical column in the periodic table. There are two notations for designating the group of elements.
Group
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Are elements which have the properties of both metals and nonmetals.
Metalloids
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Have a distinguishing electron that completes the p subshell (except He with 1s2 ).
NOBLE-GAS ELEMENTS
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Have the distinguishing electron partially or completely fill the s and p subshell.
REPRESENTATIVE ELEMENTS
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Have the distinguishing electron in the d subshell.
TRANSITION ELEMENTS
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Have distinguishing electron in an f subshell.
INNER TRANSITION ELEMENTS
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States that when elements are arranged in order of increasing atomic number, elements with similar chemical properties occur at periodic intervals.
PERIODIC LAW
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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)
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is the minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion.
IONIZATION ENERGY
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the energy needed to remove the first electron from a neutral atom
first ionization energy
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the energy needed to removed the second electron, and so forth.
second ionization energy
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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
