Basic Chemistry I Vladimíra Kvasnicová. Composition of Matter organic / inorganic compound = a...
-
Upload
christiana-mcgee -
Category
Documents
-
view
221 -
download
0
Transcript of Basic Chemistry I Vladimíra Kvasnicová. Composition of Matter organic / inorganic compound = a...
Basic Chemistry IVladimíra Kvasnicová
Composition of Matter
• organic / inorganic
compound = a substance formed by chemical reaction;it consists of elements in fixed proportions
element = a substance that cannot be decomposed into simpler substances; it consists of atoms with a same number of protons (number of neutrons may vary)
--------------------------------------------------------------- atom = the smallest part of an element that can
exist chemically molecule = the smallest part of a chemical
compound that can take part in chemical reaction
Composition of Matter
structure of atom• nucleus: protons (p+) + neutrons (n0)• „cloud“ of electrons (e-)
• mass number A (= nucleon number) • proton number Z (= atomic number)• neutron number N• electroneutrality• nuclide• isotopes
Composition of Matter
• inorganic mater oxygen (O) 50% silicon (Si) 25% aluminium (Al) 7% iron (Fe) 5% calcium (Ca) 3%
90%
sodium (Na) potassium (K) magnesium (Mg) hydrogen (H) titanium (Ti) 0,6%
• organic mater„compounds of carbon“
C, O, H, N
carbon (C) oxygen (O) hydrogen (H) nitrogen (N) phosphorus (P) sulfur (S)
• air, blood plasma
Distinguish
• isotopes = atoms having the same proton number but different mass number (isotopes of carbon: 12C, 13C, 14C)
• element = a substance composed of atoms havingthe same proton number (element consists of various isotopes)
• nuclide = a substance composed of atoms havingthe same proton and mass numbers(substance containing only 12C = nuclide called carbon „12“)
• atom / molecule / ion(monoatomic, polyatomic - binary, ternary)
Exercise
• nuclide: AZX
• make groups of:a) isotopesb) the same elementsc) the same nuclides
X 1 2 3 4 5 6 7 8
A 127 235 123 131 238 222 234 125
Z 53 92 53 53 92 86 92 53
Exercise
• nuclide: AZX
• make groups of:a) isotopes: iodine, uraniumb) elements: iodine, uranium, radonc) the same nuclides: 3, 8
X 1 2 3 4 5 6 7 8
A 127 235 123 131 238 222 234 123
Z 53 92 53 53 92 86 92 53
Calculate number of neutrons of 127I
n0 = 74
Memorize
symbols and names of elementsuse flash cards
The figure is found at http://www.corrosionsource.com/handbook/periodic/periodic_table.gif (September 2007)
Symbol Latin name English name
Na Natrium sodium
K Kalium potassium
Sn Stannum tin
Pb Plumbum lead
Sb Stibium antimony
W Wolframium tungsten
Fe Ferrum iron
Cu Cuprum copper
Ag Argentum silver
Au Aurum gold
Hg Hydrargyrum mercury
Composition of Matter
structure of atom – arrangement of electrons
• four quantum numbers
orbital = a region of space in which an electron is most likely to be found
• principal shells → energy• subshells → shape of orbitals• degenerate orbitals → space orientation• spin (rotation) of electrons
Shapes of orbitalsss
ppxx ppyy ppzz
Shapes of orbitals
ddxy ddyz ddzx
ddx 2 – y 2 ddz 2
Composition of Matter
structure of atom – arrangement of electrons
• Pauli´s exclusion principle= no two electrons in the atom can have the same set of quantum numbers
• Hund´s rule= electron will not enter an orbital containing another electron if an empty orbital of the same energy is available
Energy of orbitals
The figure is found at http://www.corrosionsource.com/handbook/periodic/periodic_table.gif (September 2007)
Composition of Matter
structure of atom – arrangement of electrons
• ground / excitated state• valence electrons• radicals
• electronegativity = a measure of the ability of an atom in a molecule to draw bonding electrons to itself
• chemical bonds
The figure is found at http://www.corrosionsource.com/handbook/periodic/periodic_table.gif (September 2007)
the arrow showes increase of
electronegativity
Inorganic Compounds
Oxides anion: O-II
• acid-forming: nonmetal / oxygen use multiple prefixes (mono, di, tri,...)
• base-forming: metal / oxygen use sufixes –ous / -ic or (oxidation state)
• amphoteric
MnO2, N2O, BaO, CO, K2O, SO2, FeO, Cu2O, CaO
Inorganic Compounds
Peroxides anion: O2-2 O-I
• s1 elements (hydrogen and alkali metals): M2O2
• s2 elements (alkali earth metals): MO2
sodium peroxide magnesium peroxide
barium peroxide potassium peroxide
hydrogen peroxide lithium peroxide
Inorganic Compounds
Hydroxides anion: (OH)-1
• basic properties (pH > 7)• strong or weak hydroxides• metal / hydroxide anion
use sufixes –ous / -ic or (oxidation state)
• ammonium / hydroxide anion
NaOH, LiOH, NH4OH, Fe(OH)3, Cu(OH)2, Ca(OH)2
Inorganic Compounds
Acids cation: H+ (pH < 7)
1) oxygen free acids
hydro-...................-ic acid
HF, HCl, HBr, HI, H2S, HCN (in aqueous solutions)
anion: -ide
• monoprotic / diprotic acids
Inorganic Compounds
Acids cation: H+
2) oxoacids the highest oxidative state per-.....-ic acid
higher (or only) oxidative state -ic acid
lower oxidative state -ous acid
the lowest oxidative state hypo-...-ous acid
anion:
-ic acid → -ate
-ous acid → -ite
Inorganic Compounds
Saltsare formed by neutralization:
acid + hydroxide → salt + water
cation: metal or NH4+
derived from the hydroxide (= cation of the hydroxide)
anion: oxygen-free or polyatomic anion derived from the acid (= anion of the acid)
Inorganic Compounds
Make groups of compounds:
Na2O, HCl, CO2, Na2O2, Ca(OH)2, KClO, HCN, HNO2,
H2S, H2O2, BaO2, PbO2, H2SO3, KOH, MgSO4, NaF,
NH4HCO3, HI, Al(OH)3, HIO4, CdS, MgO2, NaH2PO4
? oxides hydroxides peroxides acids salts