Download What does the Periodic Table tell us?

Name ____________________________________Date___________________________Hr______________
Notes – Atoms & the Periodic Table/Ions and Isotopes
What’s an atom?
 The smallest particle of matter that still has all of the properties and characteristics of
__________________________________.
 A copper atom is the smallest particle of copper that still has all of the
__________________________________.
 ________________________ – the perpetual movement of particles (jiggling atoms) named after
Robert Brown (Scottish botanist).
What does an atom look like?
 An atom is mostly empty space and contains what we call subatomic particles. They are
_______________________________________________.
 The ________________________ are located in the Nucleus, which is at the center of the atom.
 The electrons are located _____________________________ in what we call the electron cloud.
 Each subatomic particle has its own defining characteristics. They are outlined in the following
chart:
Name
Symbol
Charge
Rel Mass
Location____
__________
e1- (negative)
1/1840
Electron Cloud
__________
p+
1+ (positive)
1
Nucleus
__________
n
0 (no charge)
1
Nucleus
Draw a model here:
What’s a periodic table?


The periodic table is where we find elements. It is organized
like a ______________________.
The elements are placed in specific places because of the way
they ______________________.
What does the Periodic Table tell us?
 Each box represents an element. Each box contains. . .
1.
Atomic Number
 The smaller number with no _____________________
 Represents/determines the number of protons and electrons present in a
______________________________
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increase from top to bottom and from ______________________
If the atomic number is 2, the atom has ____electrons and ____ protons
If the atomic number is 10, that atoms has …
o i.e.
Potassium
39.098
K
19
o Potassium has ____protons and when neutral, ____ electrons.
2. Atomic Mass Number
 is the ___________________ with a decimal place and is measured in amu (atomic mass
units)
 This number gives us the number of __________________ in an atom
 To find the number of neutrons, we have a simple formula:
o __________________________________
3. Chemical symbol
 some have ___________ letters – always capitalized
 some have two letters – first letter always capitalized, second
letter is ____________________
 some have three letters – these are all man-made and may get
renamed
 some symbols are based on ___________________
o Ex) Aurum – gold – Au
Ferrum – iron – Fe
 Any element with an atomic number greater than ____ is man-made (created in a lab)
Why is there usually a decimal place in the atomic mass number?
 It is due to _________________________
 Isotopes – atoms of the same element with the same # of ____________ but a different #
of _____________
 the mass number is an estimate of all of the possible isotopes of each element
o example: C-12 has 6 neutrons, C-14 has 8 neutrons – C-12 is more often found in
nature so the atomic mass of C is 12.011, which is closer to
_________________________
How is the periodic table divided?
 Into Metals, Nonmetals and Metalloids or into Families and Periods (Rows/Columns).
Types
1. _________________
 are located to the left of the zigzag (exceptions: H and metalloids)
 properties include:
o have _______________(shine)
o can be stretched and shaped
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o conduct ________________________ very well
2. Nonmetals
 are located to __________________ of the zigzag (exceptions: metalloids)
 Properties include:
o ______________________
o poor conductors of heat and electricity
3. Metalloids/Semi-metals/Semi-conductors
 along the zigzag (B, Si, Ge, As, Sb, Te, Po)
 Properties include:
o some ________________________________________________
o not as good of conductors as metals but ___________________
_________________________________________________________
Families Vs. Periods (Rows versus Columns)
1. Rows/Periods
 are called _____________________
 are horizontal (side to side)
 elements in the same row/period _________
_________________________________________
 there are ____ of them on the periodic table
2. Columns/Groups
 are called groups or ______________
 are vertical (up and down)
 elements in the same group/family ________________________________
 there are ____of them on the periodic table
o Ex) Li, Na, K all have a similar ____________________ with water (H2O). They all
create an explosion that releases hydrogen gas (H2). Therefore, they are stored
with oil, not water.



Elements in the same group/family have the same number of
__________________electrons
Valence electrons – the number of electrons in an atom’s _________________ energy
level
o Ex) argon (Ar) versus neon (Ne)
Atoms want to achieve a filled outermost
energy level – we call this an
__________________ if the energy level
contains 8 valence electrons.
Are the groups named?
 Each family of elements group has its own name.
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Families
_______________________________
 Group 1 elements (except H)
 Have ___ valence electron
 Are the most active metals
 Tend to react with ____________ elements (halogens)
Alkaline Earth metals
 Group 2 elements
 Have _________________________
 Less reactive than alkali metals but are still reactive
 Tend to react with ____________________________
Transition metals
 group 3-12 on periodic table
 those families that we ___________________________
 Metals, but different from alkali or alkaline earth metals
 Most have ____________ valence electrons
 Includes mercury (Hg) – the only ___________metal at room temperature
Halogens
 Group ________ elements
 Some are gases, Br is liquid, and some are __________________
 Have 7 valence electrons
 Tend to react with __________________ elements (alkali metals)
_____________________
 _____________________ elements
 He has 2 valence electrons
 Ne, Ar, Kr, Xe, Rn all have 8 valence electrons
 Are ___________________ since they already achieved
an “octet”
 Contribute to less than 1% of earth’s atmosphere
o O2 (21%) and N2 (78%) contribute to most of
the atmosphere.
***Rare-Earth Elements
 includes elements at __________________ of periodic table (periods 6 and 7)
 first row = lanthanoid series- tend ____________________________
 second row = actinoid series – most are _________________ (transuranium elements) and
_______________________
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Names and symbols
 You will become familiar with the most commonly used elements and their symbols
Name
____________
Boron
Calcium
____________
Chlorine
Copper
____________
Symbol
Al
B
Ca
C
Cl
Cu
He
Hydrogen
____________
Nitrogen
Oxygen
____________
Gold
H
Fe
N
O
Na
Au
Bohr Model

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

We can use the periodic table to draw Bohr
Models. These are also referred to as
____________________________.
In these models we represent the protons,
neutrons, & all the electrons.
We already know that _________and neutrons
are located in the nucleus at the
_________________.
The electrons are located in the electron cloud in
energy levels
 1st level holds ____________
 ___________
 3rd 18e 2n^2
Fill in the following
diagram:
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Lewis ( Dot) Diagrams:
 Electron dot diagrams are structures that show the valence electrons
____________________________
 Valence electrons are the electrons in the outmost shell and can be determined
by looking at ______________________ on the periodic table
 Groups IA—VIIIA
o If an element is in group IA it has_____ electron in its valence shell.
o If an element is in group VA, it has ____ electrons in the valence shell.
 To draw the diagram:
o Write the ____________ down
o Place dots around the symbol, one on
________________ and then begin to pair them

Draw Lewis dot for the first 20 elements.
o We use Lewis dot structures to look at the
valence shell configuration because that is
where the bonding of atoms takes place!
Notes – Ions and Isotopes
Why is there usually a decimal place in the atomic
mass number?
 It is due to _____________________.

Isotopes –
o
Remember: Protons and neutrons have a
relative mass of _____, and electrons are
______, so e- ________________
__________________________ when
determining the mass
o
Since most of the mass of the element is
from __________
_______________________, changing the
number of neutrons changes the
____________________________

To determine the atomic mass, scientists take an
_____________ mass of __________ isotopes of
that atom. This gives us decimal places.

When identifying isotopes, the ________________________ is given.
o The mass number is a _______________________________
o Example:
Carbon-12 has a mass number of 12.
 How many protons does it have? Why?
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
How many electrons does it have? Why?


How many neutrons does it have? Why?

Carbon-14 has a mass number of ______
 How many p+ does it have?

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How many e- does it have?


How many neutrons does it have? Why?

When scientists take the average of these masses to determine the _____________________, they also consider
which is _______________________________ in nature.
o
C-12 is found more often in nature so the atomic mass of C is 12.011, which is closer to 12 than 14
***** IN SUMMARY *****

____________________ is a whole number and only for one isotope of that atom

____________________ has decimal places b/c it’s an average of the masses of all isotopes.

_____________________ are atoms of the same kind (so they have the same # p+ and e-), but have
different #s of neutrons.
What happens if we don’t have the same number of p+ and e-?
 Then we no longer have a __________________ atom.
o Neutral atoms have _________ CHARGE
o They have the same number of ________________ particles as _________________ particles. (these
cancel each other out!)
 Example:
Oxygen has an atomic number of ________.
A neutral atom of oxygen has _________________
So… +8 + -8 = 0
 In order for an atom to not be neutral, the number of ________ changes, the numbers of
___________________ remain the same. We call this an ______________
o Ion
Example:
o Oxygen commonly has a -2 charge.
o Oxygen always has ____________________
o +8 + -x = -2
o X = _________
o This means there are ______________ in an ion of oxygen.
o Symbol= O2- or O-2

Example:
o Boron commonly has a +3 charge.
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o
o
o
o
o
Boron always has ____________________________
Equation: ________________________
This means there are _____________________ in an ion of boron.
Symbol: ______________

Example:
o If an atom has 7 protons and 10 electrons, what is its charge?


Negative ions are called ________________.
Positive ions are called _________________.
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