full set of unit 8

name the 8 atomic theorists

1. Democritus

2. John Dalton

3. Dimitri Mendeleev

4. JJ Thompson

5. Ernest Ruthford

6. Niels Bohr

7. Louis De Broglie

8. Erwin Schrödinger

what is Democritus known for?

He came up with the theory that matter is made up of indivisible particles called atoms

What is John Dalton known for?

He came up with the modern atomic theory and is known for his billiard ball model

What is Dimitri Mendeleev known for?

Came up with the first periodic table

What is J.J. Thomson known for?

He discovered the electron and is known for his plum pudding model

What is Ernest Rutherford known for?

He proved the existence of protons and the nucleus and proposed the existence of neutrons, and is known for his nuclear model

What is Neils Bohr known for?

He is known for his bohr diagram model

What is louis de Brogile known for?

He is known for his wave model that shows there can only be a certain amount of energy in the orbit, and proposed that electrons can be waves or particles

what is Erwin schrodinger known for??

He is known for his electron cloud model that is based off the wave model, it uses math to explain how electrons behave. Electrons are found in the nucleus and the more denser it is the higher the probability of finding an electron is

What charge and mass does electrons have

has a negative charge and a mass of 0

What charge and mass does protons have?

has a positive charge and a mass of 1 amu

What mass and charge does neutrons have? and what is it responsible for?

has a neutral charge and a mas of 1 amu, it is responsible for isotopes t

what does the atomic # equal?

the # of protons

What are isotopes?

An element with the same number of protons but different number of neutrons

What is the idea of the line spectra?

It show that electrons can move between energy levels by emitting energy, and since energy is quantized it proves the existence of energy shells

what does the 2 stand for in 2p_y

its the 1st quantum number and it stands for the shell and energy level; if n=1 then it is closer to the nucleus and has a low energy while if n=7 then it is farther to the nucleus and has a higher energy level

what does the P stand for in 2p_y

it is the 2nd quantum number and it stands for the shape the orbital it is

what does the y stand for in 2p_y

it is the 3rd quantum number and it stands for the orientation of the orbital

To find the charge of an element

minus protons with electrons

how do you find the charge of nucleus

use the number of protons

Does the number of p+ change in isotopes

it never changes only neutrons

what are core e-?

they are e- in closed shells where they match the e- config of the closest noble gas

what are valance electrons

e- in the outermost shell

what does each letter stand for in 2p⁶?

2= the energy level or shell

p= the shape of orbital

6= number of electrons

what are shells?

it shows the energy level

What are subshells

types of orbitals

What are orbitals

orbitals are within subshells and it holds electrons

e- config exceptions are?

Cr and Cu; this is because atoms like to be half filled or fully filles as they are more stable

what is isoelectronic?

when the e- config matches

why do we remove e- from p then s then d?

because it requires less energy to remove e- from that are farther

what does families/groups refer to?

columns

what does periods refer to?

rows

what are the 5 main families/groups?

1. alkali metals

2. alkaline earth metals

3. transition metals

4. halogens

5. noble gases

describe alkali metals

1. very reactive

2. reactivity increases going down

3. form 1+ ions

describe alkaline earth metals

1. less reactive then alkali metals

2. reactivity increases going down

3. forms 2+ions

Describe transition metals

1. exceptions Cr and Cu

2. d orbitals are filled last

3. multivalent

Describe halogens

1. very reactive

2. reactivity increases going up

3. forms 1- ions

describe noble gases

1. full outershell

2. the most stable elements

3. poor reactivity

describe hydrogen

share properties with different families

properties of metals (hint: 6 points)

1. malleable

2. ductile

3. shiny

4. good conductor

5. loses electrons and forms cations

6. solid; except Hg

Properties of Non-metals (hint: 5 points)

1. gases

2. brittle solids (except Br)

3. poor conductors

4. dull

5. shares/gains electrons forming anions

whats a trend?

a trend is a general relationship with many exceptions

what are the 4 principles of attraction and repulsion

1. e- and p- are attracted to each other as opposite charges attract

2. e- and e- in the same subshell repel due to electron repulsion

3. e- in larger orbitals have weaker attraction due to shielding which happens when inner e- in other shells are blocking the attraction

4. more p- allow there to be more attraction due to higher Z_eff

what is Zeff?

Zeff means the effective nuclear charge and its shows the amount of pull protons/nucleus have on electrons

what is atomic radius

the distance between the nucleus and valance e-

how does the atomic radius change across a period; left to right?

It decreases

How does the atomic radius change down a group?

it increases

What is the ionic radius?

the atomic radius of an ion

why doe cations have a smaller ionic radius than their neutral atoms?

its smaller because they lose a electron shell

why do anions have a bigger ionic radius than their neutral atoms?

its bigger because they experience e- repulsion

what is ionization energy?

it is the energy required to remove an electron

why are metal larger atoms?

e- are farther from nucleus and has a weak attraction towards it

why are nonmetals smaller atoms?

e- are closer to nucleus as there is a stronger attraction pulling e- closer to nucleus

what cause higher IE?

1. e- are closer to nucleus

2. higher Zeff

how does IE change across a period?

it increases

how does the IE change going down a group?

the IE decreases

why does metals have a low IE?

1. e- are farther from nucleus

2. weaker attraction (lower Zeff)

what is electronegativity?

the attraction between shared electrons in bonds and how strong the pull atoms have on e-

which atoms have no EN value?

noble gases

How does the EN change across a period?

it increases

How does EN change down a group

it decreases

what is metallic character?

how easy it loses e- and how well it behaves like a metal

how does the metallic character change down a group?

it increases

how does metallic character change across a period (right to left)

it increases

what are the three types of intramolecular bonds

1. ionic bond

2. covalent bond

3. metallic bond

what is intramolecular bonds?

its occurs within molecules/compounds/crystals

what happens to electrons in ionic bonding?

electrons go from low EN and IE to high EN and IE

what types of structure do ionic bonds form?

they form crystal lattices which have strong attraction making ionic bonds have high MPs

what is a non-polar covalent bond?

when electrons are shared equally

how do covalent bonds form?

form when electron clouds overlap forming shared electron pairs

what is a polar covalent bond

when electrons aren’t shared equally

what does a polar covalent bond create?

it creates partially charged atoms

which atoms becomes partially positive and partially negative?

partially positive= low EN

partially negative= high EN

what is a dipole? and how is it formed?

a dipole is when one side is partially positive while the other is partially negative, it is formed when electrons aren’t shared equally and when one atom has a higher EN than the other

What are metallic bonds?

is when there’s a sea of electrons that are delocalized, and are good conductors and malleable, forming metallic crystals

what are lewis structures?

shows the amount of valance e-

what do metals show in lewis diagrams?

the dots represent the number of electrons that need to be lost to gain a full octect

what do non-metals in a lewis diagram represent?

the unpaired e- represent the number of e- that need to be gained to form an octect

exceptions for lewis diagrams

1. H can only have one bond

2. B does not need a full shell

   1. 3rd and 4th rows can have an expanded octect

How does IE show the reactivity of metals:?

metals lose electrons so the lower the IE the more reactive it is

how does EN show the reactivity of non-metals?

non-metals react by gaining or sharing electrons so the higher the EN the more reactive it is

what is electrostatic forces?

is an attraction or repulsion between charged atoms

how do you tell which pair has a stronger attraction?

by its ionic charge or atomic radius

what are intermolecular forces?

forces that describes how molecules react with each other

what is a difference between intermolecular forces and intramolecular forces?

Intermolecular forces are much more stronger

what is london dispersion force?

it is the weakest force it is always present in bonds

when does london dispersion occur?

it occurs when two temporary non-polar bonds come together and form a temporary dipole where the electron cloud shifts due to electrostatic attraction and repulsion

how does the atomic number affect the london dispersion force?

the higher the atomic number the stonger the london dispersioon force is

what happens when the LDF is only present?

it will have a low MP and BP

In london dispersion forces when will substances have a high MP and BP? (hint:chain)

more electrons= stronger attraction=stronger force=more energy needed= higher MP and BP

what is a diploe-dipole interaction?

occurs when two polar molecules come together and the opposite charges are attracted

How is the MP and BP for dipole-dipole interactions?

the stronger the attraction the more higher the MP and BP is

what is hydrogen bonding

its a specific type of a dipole-dipoles interaction that always has to involve hydrogen

when does hydrogen bonding occur?

occurs when attractive forces between hydrogen is covalently bonded with EN atoms: N, O, and F

Does hydrogen bonding have a low or high MP and BP?

hydrogen bonding has a high MP and BP

why does the MP and BP increase going down halogen family?

Have more electrons, larger AR, stronger london diseprsion force, meaning more energy needed

why does the MP and BP decrease going down alkali metal family?

larger AR, weaker metallic bonding, meaning less energy needed