CHEM 121 Overview Part 1

MATTER CLASSIFICATION SUMMARY

MIXTURES Heterogeneous mixture – components making up the mixture separate out Sand in water Homogeneous mixtures are also called solutions. No separation of components can be detected. Sugar in coffee Soda drinks

PHYSICAL & CHEMICAL PROPERTIES AND CHANGES PHYSICAL PROPERTIES OF MATTER Can be observed or measured without attempting to change the composition of the matter being observed. Examples: color, shape and mass PHYSICAL CHANGES OF MATTER Take place without a change in composition. Examples: freezing, melting, or evaporation of a substance (e.g. water) CHEMICAL PROPERTIES OF MATTER Can be observed or measured only by attempting to change the matter into new substances. Examples: flammability and the ability to react (e.g. when vinegar and baking soda are mixed) CHEMICAL CHANGES OF MATTER Always accompanied by a change in composition. Examples: burning of paper and the fizzing of a mixture of vinegar and baking soda

SUBATOMIC PARTICLES Nucleus contains protons are neutrons. Protons carry a +1 electrical charge and have a mass of 1 atomic mass unit (u). Neutrons carry no electrical charge and have a mass of 1 atomic mass unit (u). Electrons are located outside the nucleus of an atom. They carry a -1 electrical charge and have a mass of 1/1836 atomic mass unit (u). They move rapidly around the heavy nucleus.

SUBATOMIC PARTICLE CHARACTERISTICS

ATOMIC & MASS NUMBERS ATOMIC NUMBER OF AN ATOM (Z) – The atomic number of an atom is equal to the number of protons in the nucleus of the atom. MASS NUMBER OF AN ATOM (A) – The mass number of an atom is equal to the sum of the number of protons & neutrons in the nucleus of the atom. Isotopes contain same number of protons but different number of neurons

ATOMIC MASS UNIT (u or amu) and Molecular Weight An atomic mass unit is a unit used to express the relative masses of atoms. One atomic mass unit is equal to 1/12 the mass of a carbon-12 atom. A carbon-12 atom has a relative mass of 12 u. The atomic weight of an element is the relative mass of an average atom of the element expressed in atomic mass units. According to the periodic table, the atomic weight of nitrogen atoms (N) is 14.0 u, and that of silicon atoms (Si) is 28.1 u. The relative mass of a molecule in atomic mass units is called the molecular weight of the molecule. Because molecules are made up of atoms, the molecular weight of a molecule is obtained by adding together the atomic weights of all the atoms in the molecule.

MOLECULAR WEIGHT The relative mass of a molecule in atomic mass units is called the molecular weight of the molecule. Because molecules are made up of atoms, the molecular weight of a molecule is obtained by adding together the atomic weights of all the atoms in the molecule. The formula for a molecule of water is H 2 O. This means one molecule of water contains two atoms of hydrogen, H, and one atom of oxygen, O. The molecular weight of water is then the sum of two atomic weights of H and one atomic weight of O: MW = 2(at. wt. H) + 1(at. wt. O) MW = 2(1.01 u) + 1(16.00 u) = u

THE MOLE CONCEPT (continued) THE MOLE AND CHEMICAL CALCULATIONS – The mole concept can be used to obtain factors that are useful in chemical calculations involving both elements and compounds. One mole quantities of six metals; top row (left to right): Cu beads (63.5 g), Al foil (27.0 g), and Pb shot (207.2 g); bottom row (left to right): S powder (32.1 g), Cr chunks (52.0 g), and Mg shavings (24.4 g). One mole quantities of four compounds: H 2 O (18.0 g); small beaker NaCl (58.4 g); large beaker aspirin, C 9 H 8 O 4, (180.2 g); green (NiCl 2 · 6H 2 O) (237.7 g).

ATOMIC ORBITALS (continued) According to the quantum mechanical model, all types of atomic orbitals can contain a maximum of two electrons. Thus, a single d orbital can contain a maximum of 2 electrons, and a d subshell that contains five d orbitals can contain a maximum of 10 electrons.

ATOMIC ORBITALS The last descriptor of the location and energy of an electron moving around a nucleus is the atomic orbital in which the electron is located. Each subshell consists of one or more atomic orbitals, which are specific volumes of space around the nucleus in which electrons of the same energy move.

ATOMIC ORBITALS (continued) Atomic orbitals are designated by the same number and letter used to designate the subshell to which they belong. Thus, an s orbital located in a 2s subshell would be called a 2s orbital. All s subshells consist of a single s orbital. All p subshells consist of three p orbitals. All d subshells consist of five d orbitals. All f subshells consist of seven f orbitals.

FILLING ORDER & PERIODIC TABLE Notice the order of subshell filling matches the order of the subshell blocks on the periodic table, if the fill occurs in the order of increasing atomic numbers.

ELEMENT CLASSIFICATION

VALENCE ELECTRONS Valence electrons are the electrons in the outermost shell. The valence electrons determine chemical behavior and bonding behavior. The number of valence electrons is the same as the Roman numeral group number. Examples: Calcium, Ca, is in group IIA. The number of valence electrons is 2. Phosphorus, P, is in group VA. The number of valence electrons is 5.

LEWIS STRUCTURES A representation of an atom or ion in which the elemental symbol represents the atomic nucleus and all but the valence- shell electrons. The valence electrons are represented by dots arranged around the elemental symbol.

NOBLE GAS CONFIGURATIONS An electronic configuration that is characterized by two electrons in the valence shell of helium and eight electrons in the valence shell of all other group VIIIA noble gases.

THE OCTET RULE According to the octet rule, atoms will gain or lose sufficient electrons to achieve an outer electron arrangement identical to that of a noble gas. This arrangement usually consists of eight electrons in the valence shell. SIMPLE ION – A simple ion is an atom that has acquired a net positive or negative charge by losing or gaining one or more electrons.

BINARY IONIC COMPOUND FORMULAS Binary ionic compounds typically form when a metal and a nonmetal react. The metal tends to lose one or more electrons and forms a positive ion. The nonmetal tends to gain one or more electrons and forms a negative ion. The symbol for the metal is given first in the formula. NaCl, BeS, BaBr 2, Al 2 O 3

COVALENT BONDS A covalent bond is a type of bond in which the octet rule is satisfied when atoms share valence electrons. The shared electrons are counted in the octet of each atom that shares them as illustrated below for fluorine, F 2. The sharing of electrons takes place when electron-containing orbitals of atoms overlap. This is shown below for the formation of the H 2 molecule.

COVALENT MOLECULE POLARITY The shared electrons of covalent bonds are not always shared equally by the bonded atoms. Electrons of a covalent bond are attracted toward atoms of highest electronegativity.

COVALENT MOLECULE POLARITY (continued) When the resulting partial charges are distributed symmetrically in a molecule, the molecule is nonpolar. When the partial charges are distributed nonsymmetrically, the molecule is polar.

VSEPR THEORY The shapes of molecules or polyatomic ions can be predicted using a theory called the valence-shell electron-pair repulsion theory, or VSEPR theory (sometimes pronounced "vesper" theory). According to the VSEPR theory, electron pairs in the valence shell of an atom will repel each other and get as far away from each other as possible. When the VSEPR theory is used, two rules are followed: – Rule 1: All valence-shell electron pairs around the central atom are considered to behave the same regardless of whether they are bonding or nonbonding pairs. – Rule 2: Double or triple bonds between surrounding atoms and the central atom are treated like a single pair of electrons when shapes are predicted.

Molecular Shapes

INTERPARTICLE FORCE SUMMARY Ionic and covalent bonds represent two of the forces that occur between atomic-sized particles and hold the particles together to form the matter familiar to us. Other forces also exist that hold the particles of some types of matter together. These include: metallic bonding, dipolar forces, hydrogen bonding, dispersion forces.