CHEM 1127Q Lecture Notes - Lecture 17: Polyatomic Ion, Atomic Number, Nonmetal
Chemistry Final Study Guide
Chapter 1: Matter and Measurement
●Solids: has a fixed shape and volume
●Liquids: has a fixed volume but is not rigid in shape; it takes the shape of the container
●Gas: has neither a fixed volume nor a shape.
●Classification of Matter: matter can be classified in means of composition
oPure substance: each of which has a fixed composition and a unique set of properties
▪Compound: a pure substance that contains more than one element
▪Element: a type of matter that cannot be broken down into two or more pure
substances
oMixtures: composed of two or more substances in such a way that each substance
retains its chemical identity
▪Heterogeneous: non uniform mixtures are those in which the composition
varies throughout.
●Many different methods can be used to separate the components of a
mixture from one another
oFiltration: used to separate a heterogeneous solid-liquid mixture
oDistillation: used to resolve a homogeneous solid-liquid mixture
●An example is iced coffee
▪Homogeneous: uniform mixtures are ones in which the composition is the same
throughout and a solution.
●Most commonly, the solvent (the end product) is a liquid, whereas
solutes (products) may be solids, liquids or gases
●Temperature: the factor that determines the direction of heat flow
oWhen two objects at different temperatures are placed in contact with each other, heat
flows from the one at the higher temperature to the one at the lower temperature.
oThe standard unit is Kelvin
oConversions: reference the equation sheet.
●Standard Measurements: meter, kilogram, cubic meter and kelvin
●Significant figures: understanding the uncertainty of at least one unit in the last digit
oThe meaningful digits obtained a measurement
oWhen measured quantities are multiplied or divided, the number of significant figures in
the result is the same as that in the quantity with the smallest number of significant
numbers
oWhen measured quantities are added or subtracted, the number of decimal places in
the result is the same as that in the quantity with the greatest uncertainty and hence
the smallest number of decimal places
●Rules of rounding off:
o1. If the digits to be discarded are less than 500, leave the last digit unchanged
o2. If the digits to be discarded are more than 500, add one to the last digit
o3. If perchance, the digits to be discarded are 500, round off so that the last digit is an
even number
●Properties of Matter:
oChemical Properties: when the substance takes part in a chemical reaction, a change
that converts it to a new substance.
oPhysical Properties: observed without changing the chemical identity of a substance.
▪The two most common ones are melting point and boiling point
oIntensive Properties: independent of amount
▪density
oExtensive Properties: dependent of amount
▪Mass and volume
●Solubility: the process by which solute dissolves in a solvent is ordinarily a physical rather than a
chemical change
oSOLUBILITY RULES:
▪1. All nitrates compounds are soluble
▪2. All alkali metals are soluble
▪3. All ammonium compounds are soluble
▪4. All halogen compounds are soluble except with silver, lead and mercury
▪5. CHOPS are soluble except with group 1 elements, silver, lead and mercury
oSaturated:
oUnsaturated:
oSupersaturated:
Chapter 2: Atoms, Molecules and Ions
●Atoms: defined as the smallest particle of an element that can enter into a chemical reaction
●Dalton Theory:
o An element is composed of tiny particles called atoms
▪All atoms of a given element have the same chemical properties
oIn an ordinary chemical reaction, atoms move from one substance to another, but no
atom of any element disappears or is changed to an atom of another element
o Compounds are formed when atoms of two or more elements combine
●Nucleus: small, compact, positively charged and made up of protons and neutrons
oProtons: carries a unit positive charge, equal to that in magnitude of the electron
oNeutrons: an uncharged particle with a mass slightly greater than a proton
oElectrons: have almost a zero-mass value and are a negative cloud around the nucleus
oMost of the mass of an atom is concentrated in the nucleus, even though the volume of
the nucleus is much smaller than that of the atom
●Atomic Number:
oThe number of protons which is the quantity Z (Z=number of protons)
oMass Number: the sum of protons and neutrons of an element
oIsotopes: atoms that contain the same of protons but a different number of neutrons
▪Isotopic Abundance: the percent value of each atom in the compound or
molecule
●Formula: reference sheet
●Nuclear Symbol: the composition of a nucleus in terms of mass number, atomic number and
element symbol
●Atomic Mass: relative masses of atoms of different elements are expressed in these terms
oAtomic Mass Unit: amu is the standard measurements
●Avogadro’s Number: represents the number of atoms of an element in a sample whose mass in
grams is numerically equal to the atomic mass of the element
o6.022 X 10 23
●Periodic Table: the chemical properties of elements depend upon their atomic numbers, which
can be read from the periodic table
oGroups: the vertical columns
oPeriods: the horizontal rows
oMain Group elements: elements falling in groups 1, 2, 3, 4, 5, 6, 7 and 8
oTransition metals: the elements in period four, groups 3-12
oMetals: they have high conductivities and are solid in nature on the right side of the
periodic table
oNonmetals: on the left side of the periodic table and are usually gaseous
▪The periodic table is an arrangement of elements, in order of increasing atomic
number, in horizontal rows of such a length that elements with similar chemical
properties fall directly beneath one another in vertical groups
**Make sure to memorize the first 36 elements**
●Molecules (yes, again): two or more atoms may combine with one another to form an
uncharged molecule
oMolecular Formula: in which the number of atoms of each element is indicated by a
subscript written after the symbol of the element
oStructural Formula: which show the bonding pattern within the molecule
oCondensed Structural Formula: suggests the bonding pattern in the molecule and
highlights the presence of a reactive group of atoms within the molecule
●Diatomic Elements: N, P, O, S, H, F, Cl, Br, I
oElements as well as compounds can exist as discrete molecules
oNote that although molecular formulas give the composition of the molecule, they
reveal nothing about the way the atoms fit together
●Ions: the charged particles when an atom loses or gains electrons, there is no change in protons
oCations: metal atoms typically tend to lose electrons to form positively charged ions
oAnions: nonmetal atoms form negatively charged ions by gaining electrons
oMonatomic: ions that only contain one atom
oPolyatomic: ions that contain more than one atom
oIonic Bonds: ionic compounds are held together by strong electrical forces between
oppositely charged ions
oThe total positive charge of the cations in the formula must equal the total negative
charge of the anions
●Naming (here we go, shit):
oIonic Naming
▪Look through flashcards
▪Make notes with flowcharts
▪Oxonation: certain nonmetals in Groups 5 through 7 of the periodic table form
more than one polyatomic ion containing oxygen
oBinary Molecular Naming: consists of two different nonmetals and will have two words
Chapter 3: Mass Relations in Chemistry; Stoichiometry:
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CHEM 1127Q Full Course Notes
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Document Summary
Solids: has a fixed shape and volume. Liquids: has a fixed volume but is not rigid in shape; it takes the shape of the container. Gas: has neither a fixed volume nor a shape. Classification of matter: matter can be classified in means of composition: pure substance: each of which has a fixed composition and a unique set of properties. Compound: a pure substance that contains more than one element. Many different methods can be used to separate the components of a mixture from one another: filtration: used to separate a heterogeneous solid-liquid mixture, distillation: used to resolve a homogeneous solid-liquid mixture. An example is iced coffee: homogeneous: uniform mixtures are ones in which the composition is the same throughout and a solution. Most commonly, the solvent (the end product) is a liquid, whereas solutes (products) may be solids, liquids or gases. Standard measurements: meter, kilogram, cubic meter and kelvin.
