Atoms, Electrons, Periodic Table

Front 1

Describe the atomic structure of an atom.

Back 1

The nucleus is on the inside with Protons and Neutrons in it.

The electron cloud surrounds the nucleus and has electrons in it.

Front 2

Identify all the subatomic particles and their properties.

Back 2

Proton - positive in the nucleus

Electron - negative in the electron cloud

Neutron - neutral in the nucleus

Front 3

What is atomic number?

Back 3

The number of protons

Front 4

Where can the atomic number be found on the periodic table?

Back 4

Its the number on top of the element sign

Front 5

What is mass number?

Back 5

The neutrons plus the protons.

Front 6

Can you find the mass number on the periodic table? And if so where?

Back 6

No you can't.

Front 7

What is atomic mass?

Back 7

The mass of something taking into account the abundance of each thing.

Front 8

What is the equation for atomic mass?

Back 8

Atomic mass = mass A X % abundance + mass B X % abundance + ect.

Front 9

What is the difference between the Bohr Model & the Electron Cloud Model?

Back 9

The Bohr Model is far more simple than the Electron Cloud Model, it has rings surrounding the nucleus. The Electron Cloud Model has orbitals surrounding the nucleus.

Front 10

What are the 4 different atomic sublevels?

Back 10

S, P, D, F

Front 11

How many orbitals are in the S sublevel?

Back 11

1

Front 12

How many orbitals are in the P sublevel?

Back 12

3

Front 13

How many orbitals are in the D sublevel?

Back 13

5

Front 14

How many orbitals are in the F sublevel?

Back 14

7

Front 15

What is the maximum number of electrons each sublevel contains?

Back 15

S - 2

P - 6

D - 10

F - 14

Front 16

What shape is the S sublevel?

Back 16

Spheracle

Front 17

What shape is the P sublevel?

Back 17

dumbbell

Front 18

What shape is the D sublevel?

Back 18

4 clover shaped & 1 dumbbell with a hula hoop.

Front 19

What shape is the F sublevel?

Back 19

Complex

Front 20

What are valence electrons?

Back 20

Electrons on the outermost energy level.

Front 21

What is the octet rule?

Back 21

All elements want to have the most stable electron configuration, which is the configuration for the noble gases. (8)

Front 22

How are valence electrons and the octet rule related?

Back 22

The octet rules is when elements want to have 8 valence electrons.

Front 23

How would you go about starting an abbreviated electron configuration?

Back 23

Go to the closest noble gas behind the element and write that in brackets.

Front 24

What is an ion?

Back 24

A changed particle caused by in imbalance in protons or electrons.

Front 25

If an element looses 2 electrons what sign (+ or -) do you put when writing it?

Back 25

+

Front 26

How are elements arranged on the periodic table?

Back 26

Elements are arranged by rows and columns aka periods and groups/families

Front 27

What is the periodic law?

Back 27

the properties of the elements are periodic functions of their atomic numbers

Front 28

Where are metals found on the periodic table?

Back 28

on the left side

Front 29

Where are non-metals found on the periodic table?

Back 29

on the right side of the periodic table

Front 30

Where are metalloids found on the periodic table?

Back 30

between the metals and the nonmetals

Front 31

What is the difference between a row and a column on the periodic table?

Back 31

A row goes straight across and a column goes up and down.

Front 32

What is another name for a row?

Back 32

A period

Front 33

What can columns also be called?

Back 33

Groups or families

Front 34

What are the names, locations, & properties for the different families on the periodic table?

Back 34

Non-metals = hydrogen & to the right of the "stair" (reactive)

Alkali Earth = Lithium - Francium (very reactive)

Alkaline Earth = Beryllium - Radium (very reactive)

Transition Metals = the entire D block except Lanthanum & Actinium (reactive)

Metals = To the left of the "stairs" (reactive)

Metalloids = Boron, Silicon, Geranium, Arsenic, Antimony, Tellurium, Polonium. (sort of a stair case) (reactive)

Halogens = Fluorine - Astatine (very reactive)

Noble Gases = Helium - Radon (not reactive)

Front 35

What is nuclear charge?

Back 35

Nuclear charge is the attractive force between positive nucleus & electrons.

Front 36

What is the shielding effect?

Back 36

Shielding Effect is when electrons in lower energy levels shield the electrons in the higher energy levels from the full force of the nucleus.

Front 37

What is atomic radius?

Back 37

Atomic radius is half the distance between the nuclei of 2 atoms of the same element when joined.

Front 38

What is ionization energy?

Back 38

Ionization energy is the energy required to remove an electron from a neutral atom.

Front 39

What is electronegativity?

Back 39

Electronegativity is the ability of an atom to attract electrons when in a compound.

Front 40

Explain the trend and what causes Electronegativity.

Back 40

The nuclear charge ("pull") increases across a row causing the electronegativity to increase along with it.

The shielding effect increases down a row causing the electronegativity to decrease down a row.

Front 41

Explain the trend and what causes Ionization Energy.

Back 41

The nuclear charge ("pull") increases across a row causing the atomic radius (distance between middles) to decrease, this increases the ionization energy.

The shielding effect increases down a row making the ionization energy to decrease down a row.

Front 42

Explain the trend and what causes the electronegativity.

Back 42

It increases to the right because the nuclear charge "pull" increases to the right also.

It decreases down a row as the shielding effect increases down a row.