Chem Regents Test 5

Front 1

Subatomic Particles:
-Charge
-Mass
-Location

Back 1

Proton: +, 1 amu, nucleus

Neutron: neutral, 1 amu, nucleus

Electron: -, negligable, e- cloud

Front 2

Nuclear Charge

Back 2

The charge of the nucleus ONLY.

(# of Protons)

Front 3

Isotope

Back 3

An atom of the same element with a different atomic mass
(different number of neutrons)

Front 4

Calculating Average Atomic Mass

Back 4

Average Atomic Mass is given on the periodic table

It is calculated with the relative abundance of each of the isotopes

-Multiply the mass of each isotope by its abundance (change from a percent to a decimal!!!)

Front 5

John Dalton

Back 5

1803
Each element is composed of identical atoms
Atoms cant be created or destroyed
Definite proportions in compounds

Front 6

J.J. Thompson

Back 6

1896
Used a "cathode ray tube"
Discovered the electron
Theorized protons
Plum pudding model

Front 7

Ernest Rutherford

Back 7

1909
Discovered radioactivite emissions

GOLD FOIL EXPERIMENT:
Bombarded a thin peice of gold foil with alpha (+) radioactive particles, with a flourescent screen in the back
Most passed through, a few deflected
CONCLUSIONS:
-Atom is mostly empty space
-Small, dense, (+) nucleus

Front 8

Neils Bohr

Back 8

1913
Electrons exist in specific energy levels around the nucleus
The farther away from the nucleus an electron is, the higher its energy is
--Planetary Model

Front 9

Spectral Lines

Back 9

Unique for each element
Represents a specific "quanta" of energy emitted by electrons as they fall from the excited state back down to the ground state
(to jump they need energy, when they fall energy is emitted)

Front 10

Quantam Mechanical Model of Atomic Structure

Back 10

e-s have positive and wavelike properties, and can't be located
>MOST PROBABLE LOCATION of an e- is in the e- clouds
S clouds- sphere, P clouds- bowtie

Principle energy level- distance of e- from the nucleus
Sublevels (spdf)- each has a different number of orbitals. e-s are found in orbitals. 2 per orbitals. Spin in opposite directions.

Front 11

Hund's Rule for Orbital Filling

Back 11

Place 1 e- in each orbital before placing 2nd e- in any of them

Front 12

Excited VS Ground State

Back 12

An electron jumps to another level
Look for a configuration with the same number of e-, but a different configuration then normal

Front 13

Determining Number of Valence Electrons

Back 13

Total number of electrons in the outermost energy level (all electrons in all orbitals of all sublevels of the last PRINCIPAL level)

Front 14

Kernal of an Atom

Back 14

All the parts of an atom except the valance electrons
(nucleus and inner e- levels)

Front 15

Groups/ Families

Back 15

Elements in a group have similar chemical properties because they have the same number of valence electrons

Front 16

Important Groups, and Locations

Back 16

GROUP 1: Alkali Metals
- Most reactive metals, found only in bonds

GROUP 2: Alkaline Earth Metals
-Also very reactive

GROUP 17: Halogens
-Most reactive of the nonmetals

GROUP 18: Noble Gases
-Do not react because valence e- level is full

Front 17

Periods

Back 17

Elements in a period do not have similar chemical properties
They DO have the same number of occupied energy levels

Front 18

Solids, Liquids and Gases on the Periodic Table

Back 18

Solids: Most elements
Liquids: Hg, Br
Gases: All noble gases (monoatomic), and also N2, Cl2, H2, O2, F2 (diatomics) [BrI-NClHOF]

Front 19

Physical Charecteristics of Metals

Back 19

SOLID (-Hg)
Luster
Malleable & Ductile
Conduct heat & electricity

Front 20

Physical Charecteristics of Nonmetals

Back 20

SOLID, LIQUID OR GAS
Lackluster
Brittle
Don't conduct

Front 21

Atomic Properties of Metals

Back 21

Larger radius
Low ionization energy
Low electronegativity

Front 22

Atomic Properties of Nonmetals

Back 22

Smaller radius
High ionization energy
Low electronegativity

Front 23

Chemical Properties of Metals

Back 23

Create (+) Ions
Lend to lose e-

(because: larger size, e- snap off more easily)

Front 24

Chemical Properties of Nonmetals

Back 24

Form (-) ions
Tend to gain e-

Front 25

Metalloids

Back 25

"Semi metals"
intermediate properties
FOUND ON STAIRCASE
exception: Al

Front 26

Metallic Character

Back 26

Large atoms
lose e- more easily
increases as you down, decreases as you go up

Front 27

Most Reactive Metals

Back 27

First two collumns
Since the molecules are larger, the electrons are far away from the nucleus and not attracted, so they can be snapped/broken off more easily

Front 28

Most Reactive Nonmetal

Back 28

Flourine
Most electronegative atom (most able to attract e-)
4.0 on electronegativity scale

Front 29

Ionization Energy

Back 29

the energy required to get an electron away from the atom

Front 30

Trend: Atomic Radius

Back 30

INCREASES DOWN A GROUP
DECREASES ACROSS A GROUP

reason:
as you go down, it gets bigger because the nubmber of energy levels increases
as you go across it gets smaller because the increased number of protons in the nucleus pulls the energy levels in closer to the nucleus

Front 31

Trend: Ionization Energy

Back 31

DECREASES DOWN A GROUP
INCREASES ACROSS A PERIOD

reason:
the larger the atom, the less the nuclear charge pulls on the outer electron. this makes it easier for another atom to snap off it's electron

Front 32

Electronegativity

Back 32

Ability an atom has to attract e-

Front 33

Trend: Electronegativity

Back 33

DECREASES DOWN A GROUP
INCREASES ACROSS A PERIOD

reason:
Because as size of an atom increases, its nuclear charge's pull decreases and it is less able to attract electrons.

Front 34

Transition Elements

Back 34

Groups 3-12
"d" block
multiple possible charges
from colored compounds
can use d-sublevel to form bonds

Front 35

Atomic vs. Ionic radius

Back 35

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