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Science 10 AP Notes
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Science 10 AP notes including topics such as biology, chemistry, physics, and climate. Includes diagrams and practice problems. Final class grade was 94%.
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chemI
, MATTER AND ATOMS chem
matter 05 09 23
classifying . .
matter
Mixtures Pure substance
Homogenous/
solution Heterogeneous/
mechanical mixture
compounds elements
1011C covalent 101-metals metals Metalloids
Properties of matter 06 09 23
. .
Physical properties : physical appearance and composition of a substance
↳ e .
g . boiling/condensation/melting/freezing point malleability ductility , , ,
colour state
, ,
solubility ,
crystal formation ,
conductivity magnetism
,
chemical propernes :
reactivity of s
a rostance
4 ability to oure
,
flash point behavior ,
in air
,
reaction with water
,
reaction to acids reaction to heat
, ,
reaction to red/blue litmus
Atomic Theory
Dalton-1803
H
-
matter is made of atoms with a solid and uniform shape
-
can't be created , destroyed ,
or further divided O
-
atoms of the same element are identical in mass and size
Ch
-
compounds form from different elements combining
- chemical reactions change how atoms are grouped but not atoms themselves
( J
. . Thomson -
1897
-
plum pudding model or rasin our model
- + Ve
-
charged particles (electrons) are smaller than the atom
ve
-
-
-
-
electrons are embedded in spherical cloud of+ ve charge
Ernest Rutherford -
1911
-
solar system model -
-
atoms contain nucleus >
-
central +he charged relgon
-
-
-
electrons more around the nucleus in empty space
-
performed the Gold Foll Experiment with Hans Geiger and Ernest Marsden in 1911
↳ determined that atoms contain a small but dense nucleus with positive charge and low-mass electrons doing further out
↳ also determined that the space within an atom is almost
entirely empty as most of the a particles passed through the foll without lere
Niels Bohr -1913
-
-
elections
electrons
Subatomic Particles
have
can only
certain
more
energy shells/levels
between levels by gaining/emitting energy
⑩
Name Symbol charge Location
Protons Ot & nucleus
relatively equal mass (n1)
Neutrons no neutral/N/A nucleus
Electrons e - Orbitals negligible mass (n0)
D) eterming Atomic Mass
-
nucleus has a small size compared to the atom but contains almost all of the Mass
-
protons determine the element
-
atoms are neutral , p+ = e-
-
atomic number =
pr and e
-
atomic mass =
pt combined with no
neutrons = atomic mass-atomic number
2
-
, ISOTOPES, IONS, COMPOUND TYPES chem
Isotopes
-
elements with differing mass that are chemically alike
elements often have z or more Isotopes > carbon-12
(12C) and carbon 13
(C)
- -
-
Electron EnergyLevels P7 . 89 23
.
1 . Maximum Ze-
2 . Maximum Be-
.
3 Maximum Se-
Stable octet : valence shell has all be -
Bohr Diagrams
Full Bohr
Diagram-caroon
Condensed Bohr Diagram-carbon
42
Ze
-
+
p 6
xix
=
+
p
6
=
I 10 = 6
1 =
6
Valence electron ordering : 4 2
-
T Y
& 3
!
7
-
Lewis Dot Diagrams
.... p. :::
-
in ca .
-
lonic compounds Bonds
metal cation and non-metal anlon combine
-
Blanary : I elements ,
-
valence electrons from metal are transferred to the non-metal
↳ e g Nach
Nar:
. .
[Na]" [21]
-
1011C Bonds : cations and anions are held together by electrostatic force of attraction between the oppositely charged lons
↳ STRONG bonds
-
Crystal lattice : whenc onic compounds are solid the
,
loss arrange themselves to maximize attractions and minimize repulsions between the +re and-re
101s
08 89 23 . .
Ionization :
gain or loss of electrons from outer energy level/valence shell
10n : protons electrons
, particle has a charge
cations :
positivelons
↳ Metals : Usually form cations
)
↳ naming element plus 101 >
-
potassium Ion (excluding polyatomic lons)
Anions : negative cons
↳ 101-metals form anions
usually
↳ naming : change ending to ide >
-
Chloride (excluding Polyatomic 101s)
I delectronic : two or more elements with an equal number of electrons
molecular/covalent compounds 11 09 23
. .
-
combination of 2 or more non-metals
-
2 non-metals is a Gianary molecular compound
I or more pairs of electrons in
share a covalent cond
they
-
-
form covalent bonds to complete valence energy level
Types of Bonds
Single bond share 2 electrons
,
I each
Double bond share 4 electrons
,
I each
Triple bond share 6 electrons , 3 each 3
, MOLECULAR COMPOUNDS, PROPERTIES, NAMING chem
common Molecular compounds 12 .
09 23
.
Chemical Formula common name
NHz(g) Ammonia
CHi20g(s) Glucose
CizHzz Once sucrose
CHa(g) Methane
C3Hs(g) Propane
CHz COOH Acenc adid
(aa)
- posite
H20(ei water t
H low
electronegativity
·
Oz Ozone
H
(g)
CHzOH Methanol
, e)
CHsOH(e) Ethano O
H202(e) Hydrogen peroxide - -
negative
high electroneganim
·
properties of compounds -
conic vs . covalent
property IONIC covalent
Melting point High row
solubility in water check solubility chart Dissolve If polar
conductivity as solid No Ng
conductivity in solution yes NG
Bond strength Strong weak
Polyatomic Elements
Atc-Astatle 12 Iodine
-
Biz-Bromine N2-Nitrogen
C2-chlorine O2-oxygen
Fz
-
Fluorine D -phosphorus
a
Hz-Hydrogen -g -
Sulfur
Naming and Formulas for Blanary covalent compounds
mono only for second element Dihydrogen Monoxide PCls-phosphorus pentachloride
> H20
-
-
second ends in'-ide' heptaflouride
-
Tetraphosphorus decactide
-
Pe010 'sF - -triodine
I-monc 3-tri S-penta 7-hepta 9-nona Cennea Nitrogen trichloride > NCL > - 00-disulfur nexoxide
-
2 di 4-tetra 6-nexd 8-octa 10-deca
Naming and Formulas for lonk compounds
-
univalent :
only form one charge LF(s) - Lithium flouride
-
Multivalent : more than one charge possible MgBrzes) >
-
magnesium Gromide
↳ most common charge listed first ; roman numeral in name to indicate charge NaCH COOcs) - rodium acetate
,
-
polyatomic lon : more than one atom in an lon NHa Hz POt(s) + ammonium dihydrogen phosphate
alwayslst 2nd
canon anion always
Mgz (BOs) z(s) -
Magnesium borate
-
,
-
name cation with element's name roman numerals in trackets for multivalent ; anion uses first part of element name and ends in 'ide'
,
-
polyatomicl on uses name from polyatomic on table
5102c) + + (IV) Oxide
Mg (OH) c)
- magnesium hydroxide
NaHzPOp() - sodium dihydrogen phosphide
&
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