Isotopes/ Ions/ Bohr Model and More

Isotopes

• The # of neutrons can be variable for many elements. 

• Atomic # = number of protons in an atom

• Isotopes are atoms that have the same # atomic #, but different mass numbers due to a change in the # of neutrons

• Nucleus, the center of an atom, is made of protons & neutrons. 

Protons 

( + ) charged particles found in the nucleus of an atom. They determine the atomic number and identity of an element.

Neutrons

( n0 ) neutral particles found in the nucleus of an atom. They contribute to the atomic mass but not to the charge of the atom.

Electrons 

( - )charge particles that orbit the nucleus of an atom, playing a key role in chemical bonding and reactions.

Atoms can form….

ions or isotopes by gaining or losing electrons or neutrons.

What are the charge of atoms?

they don’t have a charge

What are elements defined by?

the number of protons in their nucleus

What do metals on the periodic table form?

they form positive ions

What do non- metals on the periodic table form?

they form negative ions

What do you have to do to make a positive ion?

take away an electron

What do you have to do to make a negative ion?

you add an electron

Which group of elements does not form ions?

Noble gases

How many electrons are in the first outer shell?

Two electrons

How many electrons are in the second outer shell?

Eight electrons

When you gain an electron for ex. Li how would you write it out? 

You would write it as Li-

When you loose an electron for ex. Li how would you write it out?

You would write it as Li+

Electro - negativity

is the tendency of an atom to attract electrons within a chemical bond.

What’s the trend when you across the PT for electronegativity?

Electronegativity increases across a period as the atomic number increases, leading to a stronger attraction for electrons.

What’s the trend when you down the PT for electronegativity?

Electronegativity decreases down a group as atomic size increases, resulting in a weaker attraction for electrons.

Ionization Energy

is the amount of energy required to remove an electron from an atom or ion in the gas phase.

Solve for thus problem answer: P+, N0, and e-

p* = 7. N0 7, e- = 7 =

How do you find the mass #?

Add the number of protons and neutrons in the nucleus of an atom.

How do you find the # neutrons?

Subtract the atomic number from the mass number of the atom.

How do you know how many circles you have to draw using Bohr’s model using the periodic table? 

Look at the periods of the periodic table 

Electronegativity

is the tendency of an atom to attract electrons in a chemical bond.

What’s the trend for electronegativity?

as you go across the PT from left to right, electronegativity increases, while increases as you go up the periodic table

Ionization Energy 

is the energy required to remove an electron from an atom or ion in its gaseous state.

What’s the trend for ionization?

as you go across the PT from left to right, ionization increases, while it increases while going up the periodic table

How do you find the number of nuetrons?

Subtract the atomic number from the atomic mass of the element.

Ground State

is the form that an atom is normally in

Why do electrons get exicted?

b/c of the heat and light will show (ex. color) 

Excited State

e- gets excited when it gets energy (sun, heat, fire…) and moves to a higher energy level.

As the wave length increases what happens to the frequency?

The frequency decreases, indicating an inverse relationship between wavelength and frequency.

As the wave length decreases what happens to the frequency?

The frequency increases, demonstrating the inverse relationship between wavelength and frequency.

P orbital 

• Hold’s a max of 6 electrons ( x= 2) (e-) and( z=2 )

• Groups 1-2 

S orbital

• Holds a maximum of 2 electrons (x=1) (e-) and (z=1)

• Groups 13 -18

What does the 1 stand for in 1S2?

energy level (period groups)

What does the S stand for in 1S2?

orbital

What does the 2 stand for in 1S2?

Number of electrons

Energy Levels

• As you go farther from the nucleus, electrons at higher levels have more energy & their energy.

• Electrons can jump from a higher to lower energy level if they absorb this amount of energy.

• If electrons jump from higher —- lower energy level, they give off energy, often to form of light.

Which energy level would you find the most energy? (only 4 in the context)

The fourth energy level (4s)

S orbitals are what shape?

spherical

What shape are P orbitals?

dumbbell-shaped

Aufbav Rule

electron configuration energy increases levels as you write them out.

Pavlie Ruler

when you put the arrows into box one goes up on always goes down. (spin)

Hund’s rule 

• states that electrons will fill degenerate orbitals singly and with the same spin before pairing up in orbitals.

• one in each box before you put one arrow orbital box before two goes into any. 

Energy levels

in an atom are the fixed distances from the nucleus where electrons are likely to be found. Each level corresponds to a specific energy state.

What happens with the energy levels as you get father from the nucleus?

The energy levels increase, allowing electrons to occupy higher energy states.

What energy level would have the most energy?

The outermost energy level, often referred to as the valence shell, contains electrons with the highest energy.

Atomic radius

measurement from the nucleus to the valence electrons

Nuclear charge 

is the total charge of the nucleus, determined by the number of protons present in the atom.

Atomic Mass does what of the periodic table?

atomic mass increases moving down each group and right across a period 

Transition Medals locations 

are found in the d-block of the periodic table, consisting of groups 3 to 12.

Alkali metals location 

are found in group 1 of the periodic table, excluding hydrogen. They are known for their high reactivity and tendency to lose one electron.

Alkaline earth metals location

are found in group 2 of the periodic table. They are characterized by having two valence electrons and are less reactive than alkali metals.

Post - transition metals location

are found in groups 13 to 16 of the periodic table, located to the right of transition metals.

Metalloids location 

are found along the zig-zag line on the periodic table, between metals and nonmetals. They exhibit properties of both metals and nonmetals.

Non-metals location

are found on the right side of the periodic table, primarily in groups 14 to 18. They are characterized by their lack of metallic properties and high electronegativity.

Noble gases location

group 18

Halogens location

group 17

How many orbitals and electrons are in f orbitals?

There are seven f orbitals, which can hold a total of 14 electrons.