Subatomic Particles: Electrons, Protons, and Neutrons · 2018-10-29 · Subatomic Particles:...
Transcript of Subatomic Particles: Electrons, Protons, and Neutrons · 2018-10-29 · Subatomic Particles:...
Chemistry 11 – Atomic Theory Study Guide 1
Subatomic Particles: Electrons, Protons, and Neutrons Rutherford-Bohr Model: Definitions:
• Proton: ______________________________________________________________________ • Neutron: _____________________________________________________________________ • Electron: _____________________________________________________________________
Electron Proton Neutron
Symbol Charge
Mass (amu)
Atomic Number and Mass Number
Look at K for example: _________________
_________________ 19
K Potassium 39.098
_________________ _________________ Definition:
Atomic Number: � Of an element is the _______________________________________________ of its atoms. � No two elements have the _______ atomic number. � This number defines an ________________. � Increases by ______ as you go through the periodic table (refer to periodic table)
• Number of protons = _________________________________ (in neutral atoms)
Therefore, for K: 19 protons = ______ electrons in a neutral atom.
neutral e-
= pt
Helium on = n
•
BaeDM = e
-
• - nucleus•
is
Subatomic particle in the nucleus that is tveiy chargedSubatomic particle in the nucleus that is neutralSubatomic - rely charged particle
e- pt n- I +1 neutral
1/1837 I I 1
t tightest subatomic particle
symbolAtomic #
( Whole # I
I 39Atomic mass a T Name
( decimal # ) Mass #
Mass # does not
appear in the p - table
# of ptsameelement
one
atomic # = # of e-
-19=
Chemistry 11 – Atomic Theory Study Guide 2
So how do we fill the electrons in the shells?
• We follow the rule that certain shells can hold a certain number of electrons. 1st shell: ___ e-
2nd shell: ___ e-
3rd shell: ___ e-
4th shell: ____ e- …etc. We will only focus on the first 20 elements for now! Bohr Diagram for K: Ions: • Electrons can be ______________ from an atom if enough ____________ is applied to it.
For example, Na atom → Na+
sodium atom remove e- sodium ion 11 protons 11 protons 11 electrons 10 electrons
• Ions usually form as a result of atoms having _________________________________________. • +ve charged ions have ______ electrons, while –ve charged ions have __________ electrons
Bohr Diagram for Na+:
How do we find out the number of neutrons in an atom?
Definition: Mass number: � __________________________________________________________________.
� __________________________________________________________________.
2
8
q f 4th row has 18 elements.
18
-0 • ← 4th Shell• •
= Outermost shell• •
• •= Valence shellIIslqpt • •
• @
• o
• •
removed energyneutral +
← cation
" } more pt
full Valente shell = stable
lost gainedcation anion
+
• •
Charge• • Include E J
•
• HptDog for Tons
D O
Whole decimal
Aatomic mass
Total # of Pt and he
can increase by more than one as you move
left to right In the p - table .
Chemistry 11 – Atomic Theory Study Guide 3
• By convention,
________ number 39 _________ number 19K
Example using K: How many neutrons are present in an atom of K that has mass number = 39? mass number = number of protons + number of neutrons number of neutrons = = =
Isotopes
• Not all atoms of the same element contain the same number of ___________ (remember
number of protons determines the identity of elements, NOT the number of neutrons). Definition:
Isotopes: � _______________________________________________________________________
Example: Carbon, C has three naturally occurring isotopes: C-12, C-13, C-14
Electron Configuration
Definition: Electron Configuration:
• _______________________________________________________________________
_______________________________________________________________________ 4 types of shells:
• s orbitals can hold ___ e- • p orbitals can hold ___ e- • d orbitals can hold ___ e- • f orbitals can hold ___ e-
Top # is
Mass= # pt + * n
falways bigger
= # ptAtomic -
-
# n = 20
NeutralMass # - # pt atom
( # pt + # n ) - # Pt f I \39 - 19 = 20 V
Changpet change e-change
n
d t tNew element ION Isotope
neutron
Atoms having the same # of pt but not n
- - -C*5
It *mass #
A description Ot Which orbitals in an atom contain
e- and how many e-
are in each orbital .
Chemistry 11 – Isotope Calculation Study Guide !
!
Isotope Calculation Complete the following table:
!!!" or C-12 !!!" or C-13 !!!" or C-14
# of p+
# of e-
# of n
Atomic # (# of p+)
Mass # (# p+ + n)
Atomic mass Why is the mass number of element different from the atomic mass? The mass number is a whole number which represents sum of # of p+ and n but atomic mass is usually a decimal number which represents the molar mass of the element. Definition: Molar mass: ________________________________________________________________________ e.g., Molar mass of Cl is ____________. Where did this number come from?
• Scientific data tells us that there are two isotopes of chlorine Cl-35 and Cl-37. 75.77% of the element is Cl-35 and 24.23% of it is Cl-37.
!"#$%!!!"##! = ! !"#$%&'(!!"!!"#$#%& !!!(!"##!#!)
e.g., What is the molar mass of boron, given that there are:
• 18.8% of B-10 • Rest is all B-11
e.g., What is the molar mass of magnesium, given that there are:
• 78.99% of Mg-24 • 10.00% of Mg-25 • Rest is all Mg-26
!
°
J6 6 6
66) Gp µ ,6g6 6 6
12
13L14
= C decimal found in table ) 12.0M-
µAtomic mass
Mass of one mole of particles .( glmoi ) I
35.5
Formula I Sigma = Add up all terms ←hj too
0.7577not to
CI - 35 Cl - 37
MM lol ) = ( 0.7577×35 ItC.2423×37 )p
= 26.
5195 +2423%9651 = 35 . 4846
=
B - I ,us
35.591mg
B - 10
MMLB )= C.188 x 10 It
C. 812×11 )10040 - 18.8610 = 1.88 t 8.932
= 81.2010 =
10.812 I 10.89mmol=
. 812 fuSEIDPT
I
MMCMGLTReported 243
↳ toooo= C.7899×24It C.1000×25 ) t
(0.101×26)- 178.99010 = 24.3203 = 24.39 Imo )
-10.000/011.0/0/0
= 0.1101
#ptyt # n
X =
Mass Number0846kV=360 84-36=48 I
&zFBr351-45=80 35 = I' FBI.
=530 127-53=44mo
If Co 271-32=59 =④ I88 30+36=66 30 = ③ 300
Yoo 0mF't 48 =480 112-48=64 ⑧morg%8qSr2t501-38=88 38 =m0r② It FITE"
127 52 = ⑤ D¥fRh3t 45 = 45 58
' 3FAs3-
75 = 33 36
e) 65.591mm
f I 91.3 9lmo1
g) 95.9mmol
IHe
. Finish Review WIS
periodicTable
!
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