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Subatomic Particles: Electrons, Protons, and Neutrons · 2018-10-29 · Subatomic Particles:...

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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 Bae DM = e - - nucleus is Subatomic particle in the nucleus that is tveiy charged Subatomic particle in the nucleus that is neutral Subatomic - rely charged particle e- pt n - I +1 neutral 1/1837 I I 1 t tightest subatomic particle symbol Atomic # ( Whole # I I 39 Atomic mass a T Name ( decimal # ) Mass # Mass # does not appear in the p - table # of pt same element one atomic # = # of e - -19 =
Transcript

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

!

↳ Quiz next mon

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