chapter 2 atoms chemistry b11. matter anything that occupies space and has mass pure substances...
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Chapter 2
Atoms
Chemistry B11
MatterAnything that occupies
space and has mass
Pure substancesFixed composition, cannot
be more purified
MixturesA combination of two
or more pure substances
PhysicallySeparable into
ElementCannot be
subdivided by chemical or
physical means
CompoundsElements united
In fixed ratios
HomogeneousmatterUniform
Compositionthroughout
Heterogeneousmatter
Nonuniformcomposition
CombineChemically
To form
Element: is a substance consists of identical atoms.
Cannot be divided by chemical & physical methods.
Carbon, Hydrogen, Oxygen
116 elements – 88 in nature
Compound: is a pure substance made up of two or more elements in a fixed ratio by mass.
H2O (Water): 2 Hydrogen & 1 Oxygen
CO2: 1 Carbon & 2 Oxygen
20 million compounds
Compounds Formula
Identifies each element Ratios
H2O
CO
H
O
2=
1or 2 : 1
C
O
1=
1or 1 : 1
O
H HH2O
Molecularformula
Structuralformula
Ball-and-stickmodel
Space-fillingmodel
Molecular models
C
H
H
H
HCH4
Mixture: is a combination of two or more pure substances.
Homogeneous: uniform & throughout
Air, Salt in water
Heterogeneous: nonuniform
Soup, Milk, Blood
Mixtures
Law of conservation of mass:
C + O CO
1. All matter is made up of very tiny, indivisible particles (atoms).
2. All atoms of a given element have the same chemical properties.
3. Compounds are formed by the chemical combination of two or more different kinds of atoms.
4. A molecule is a bound combination of two or more atoms.
Dalton’s Atomic theory
Monatomic
Ar He
Diatomic
N2 O2
Polyatomic
Element:
S8
Atom
Atom
Nucleus: positive charge
Atoms are neutral.
Atomic mass unit (amu) = 1.6605×10-24 g
mass of proton = 1 amu
mass of neutron = 1 amu
mass of electron = 5.48×10-4 amu
Atom
Mass number (A): Protons + Neutrons
Atomic number (Z): Protons
C12
6
Mass number
Atomic number
Isotopes
Isotopes: atoms with the same number of protons and electrons butdifferent numbers of neutrons.
different mass numbers
C12
6 C13
6 C14
6
6 P + 6 N 6 P + 7 N 6 P + 8 N
Almost the same properties
Atomic Weight
Atomic weight: of an element is average of the masses (in amu) of its isotopes found on the Earth.
Cl Cl35
17Cl37
1734.97 amu 36.97 amu
(75.77/100 × 34.97 amu) + (24.23/100 × 36.97 amu) = 35.45 amu
Cl17
35.45
Atomic number
Atomic weight
Main-group elements: 1A to 8A
Transition elements: 1B to 8B (3 – 12)
Inner transition elements: between B3 & B4 (58 to 71 and 90 to 103)
Column: same properties (main group)
Row or Period
Group 1A: Alkali metals
Li-Na-K-Rb-Cs-Frtoo reactive, unstable, solid metal
2Na + 2H2O 2NaOH + H2
2Na + Cl2 2NaCl
Group 2A: Alkaline metals or Earth metals
Be-Mg-Ca-Sr-Ba-Rareactive, solid metal
Group 7A: Halogens
F-Cl-Br-I-Atreactive, colored, gas, nonmetal
Group 8A: Noble gases
He-Ne-Ar-Kr-Xe-Rnnon reactive, stable, gas, nonmetal
nonmetals
metals
metalloids
Classification of the elements
metals: solid (except mercury), shiny, conductors of electricity, ductile, malleable
nonmetals: solid, liquid or gas, do not conduct electricity (except graphite)
metalloids: between metals and nonmetals
to
More metallic
Mo
re m
etal
lic
Metallic properties
n=1
n=2n=3 n=4
n=5
E1 E2 E3 E4 E5
E1 = ground state: lowest energy level
Bohr model
Principal energy levels or Shells
324
183
82
21
Maximum number of electrons
Shell
Lower energy
Higher energy
Subshell: s p d f
Orbital: is a region of space and it can hold 2 electrons (max).
s px py pz
magnetic field
paired spins
s p d f
2 2+2+2=6 2+2+2+2+2=10 2+2+2+2+2+2+2=14
Subshell: s p d f
Shell OrbitalsMaximum number of electrons
1 1s 2
2 2s, 2p 2 + 6 = 8
3 3s, 3p, 3d 2 + 6 + 10 = 18
4 4s, 4p, 4d, 4f 2 + 6 + 10 +14 = 32
3
2
3d3p
3s2p
2s
Principal energy level Orbitals
En
erg
y
Ord
er
of
filli
ng
1 1s
Electrons configuration: description of the orbitals that its electrons occupy.
Orbital box diagrams
H (1)1s
1s1
Electron configuration
1sHe (2) 1s2
Li (3)
1s 2s
1s2 2s1
C (6)
1s 2s
1s2 2s2 2p2
2px 2py 2pz
Noble gas notation
Li (3)1s 2s
1s2 2s1
[He] 2s1
F (9)1s 2s
1s2 2s2 2p5
[He] 2s2 2p52px 2py 2pz
Si (14)1s 2s 3s2px 2py 2pz 3px 3py 3pz
1s2 2s2 2p6 3s2 3p2
[Ne] 3s2 3p2
Valence electrons: outer-shell electrons
Valence shell: outer shell
Cl (17) 1s2 2s2 2p6 3s2 3p5 7 valence electrons
Ar (18) 1s2 2s2 2p6 3s2 3p6 8 valence electrons
C (6) 1s2 2s2 2p2 4 valence electrons
Ne (10) 1s2 2s2 2p6 8 valence electrons
Noble gases Filled valence shells
Elements in the same column (group) have the same number of electrons in their valance shells.
The same chemical and physical properties.
For Main-group elements:
Lewis dot structure
H He Li C Cl
1A 2A 3A 4A 5A 6A 7A 8A
Main groups elements s, p
Transition elements s, p, d
Inner transition elements s, p, d, f
Atomic Size
Size of an atom: is the size of its outermost occupied orbital.
d
Ionization Energy
Li + energy → Li+ + e-
ion
Ionization energy: the energy required to remove the most loosely held electron from an atom in the gaseous state.
Ionization energy
Ion
izat
ion
en
erg
y
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