Chem104- Exam 2

Front 1

Nucleus

Back 1

dense, central part of atom containing neutrons & protons and contains most of the mass of atom & all of positive charge.

Front 2

Orbital

Back 2

Energy levels of electrons. Each energy level can have 1 or more sublevel (s,p,d,f) Each sublevel can have 1 or more orbitals

Front 3

atomic number

Back 3

number of protons in an element.

Front 4

Electron shell

Back 4

An orbit followed by electrons around the nucleus of an atom. Each shell can contain only a fixed number of electrons, each shell is associated with a particular range of electron energy, and each shell must fill completely (7) on a row before electrons can be added to an outer shell. The electrons in the outermost shell determine the chemical properties of the atom and is called the valence shell.

Front 5

Avogadro's #

Back 5

A mole- 6.02 x 10(23) atoms or molecules

Front 6

Noble gas

Back 6

chemical family that doesn't combine w/any other family. Last row on periodic table and has full outer shell.

Front 7

atomic mass unit (amu)

Back 7

Unit of mass used to describe the relative masses of atoms. 1 amu 1/12 of a carbon 12 atom and is practically equal to mass of a neutron or proton.

Front 8

atomic weight (mass)

Back 8

avg. mass of the atoms of an element compared w/an atom of carbon 12 at exactly 12 amus.

Front 9

gram-atomic weight

Back 9

mass of 1 mole of an element equal in grams to the atomic weight.

Front 10

mole

Back 10

6.02 x 10(23) atoms, molecules, or ions. There is exactly 1 mole of atoms in 12g of carbon-12

Front 11

Provisions of Dalton's Atomic Theory?

Back 11

1.Elements composed of minute, indivisible particles called atoms.
2. Atoms of same element are alike in mass & size
3. Atoms of diff. elem. have diff. masses & sizes
4. Chem. compounds are formed by union of 2 or more atoms of diff. elements.
5. Atoms combine to form compounds in simple numerical ratios such as 1-2, 1-1, 2-3
6. Atoms of diff. el. may combine in diff. ratios to form more than 1 compound

Front 12

Give the names, symbols, charges, and rel. masses of the 3 principle subatomic particles?

Back 12

1. Electron; e; -1; .0006
2. Proton; p+; +1; 1
3. neutron; n; 0; 1

Front 13

Describe the atom as conceived by Rutherford after his alpha particle scattering exp.?

Back 13

this model had the protons & neutrons in the nucleus of the atom and the electrons located around the nucleus.

Front 14

Describe atom as conceived by Neils Bohr?

Back 14

He believed that electrons had specific orbits at specified distances and didn't reside b/t orbits. Energy would be quantized for each electron and energy added to the atom could cause the electron to move to a higher orbit.

Front 15

John Dalton

Back 15

proposed a model for the nature of matter. Atomic Theory

Front 16

J.J. Thomson

Back 16

showed existence of electron through use of crookes tube (cr tube

Front 17

Goldstein

Back 17

first to observe the protons (particle and had mass; charge is positive)

Front 18

Chadwick

Back 18

discovered neutron (same mass as proton)

Front 19

Rutherford

Back 19

designed exp (gold fold) that gave insight into interior of atom.

Front 20

Bohr

Back 20

studying line spectra from h2. planetary model of atom.

Front 21

schrodinger

Back 21

used math to determine prob. of finding electron in particular area around nucleus.

Front 22

Maximum # of electrons in a given main energy level?

Back 22

2n 2

Front 23

Draw an S orbital and P orbital

Back 23

s- is one circle
p- 2 circles side by side (figure 8 sideways)

Front 24

Know electron configuration:

Back 24

s,p,d,f

Front 25

Draw diagram of any isotope of 1st 38 elements showing composition of nucleus & number of electrons in main energy levels

Back 25

s-1, p-3, d-5, f-7

Front 26

Name 3 isotopes of Hydrogen & give # of protons, neutrons, & electrons in each:

Back 26

Protium- 1 proton, 0 neutrons
Deuterium- 1 proton, 1 neutrons
Tritium- 1 proton, 2 neutrons

Front 27

Be able to tell # of protons/neutrons based on atomic # & weight.

Back 27

ex. O (atomic weight) is 15 subtract the # of protons 8 (atomic #) and you have 7 neutrons.

Front 28

Calculate # of atoms, moles, or grams from appropriate data

Back 28

notes

Front 29

Periods?
Groups/Families?
Transition elements?

Back 29

Period-row
Group- column

Front 30

1. Mendeleev
2. Moseley
3. Meyer

Back 30

mendeleev- helped form p table
Moseley- ordered p table according to atomic #
Meyer- also helped w/ p table

Front 31

Locate metals; non metals; metalloids; noble gases; alkali metals; alkaline earth, chalcogens, halogens

Back 31

metals-left side
non- right side
metalloids- stair case
alkali- 1st column
alkaline earth- 2nd column
noble gas- helium
chalcogens- oxy family
halogens-fluorine

Front 32

Describe how atomic radii vary from left to right in period and from top to bottom in group?

Back 32

decreases slightly across from l to r.
Increases down p table

Front 33

Describe changes in outer level electron structure from l to r & from top to bottom

Back 33

more electrons packed into nucleus from l to r & down the the chart increases orbitals

Front 34

Predict formulas for simple binary compounds (2 nonmetals) using p table.

Back 34

does it give away or gain electrons from its shell
(ex. Mg2+ F1-)

Front 35

Describe electron config. of transition elements (d block)?

Back 35

(ex. Fe2+Cl1--> Iron (II) Chloride

Front 36

Which metals make more than one type of cation? (need Roman numerals) non metal takes -ide ending

Back 36

(1-2) Copper, Mercury
(2-3) Iron, Tin
(2,4) Lead
(3,4)Titanium
(3,5) Arsenic

Front 37

ionization energy?

Back 37

energy needed to remove an electron.
Decreases down p table and
Increases across

Front 38

Covalent bond?

Back 38

bonds that share electrons

Front 39

Polar covalent bond?

Back 39

Don't share well. Share unequally b/c of electroneg. (occurs as you move across p. table
Creates dipoles

Front 40

polyatomic ion?

Back 40

Single unit, rarely separated. elements of opposite charges
(anions or cations)
Cations- Ammonium Hydronium

Anions- Phosphate, Carbonate, Sulfate, Cyanide, Hydroxide, Nitrate

Front 41

oxidation-reduction?

Back 41

oxi- loss of electrons or increase in oxy state

reduction- gain of electrons or decrease in oxy state

Front 42

electronegativity?

Back 42

ability of an atom to get an electron and hang on to it.

Front 43

Ionic bond?

Back 43

Require transfer of electrons; formed b/t 2 charged atoms (cations & anions)

Front 44

1. non-polar covalent bond
2. coordinate covalent bond

Back 44

1. (ex. methane) electrons shared equally
2. also called dipolar bond

Front 45

oxidation #?

Back 45

tells whether the element in a compound gives away or takes electrons.

Front 46

valence electrons?

Back 46

highest energy s & p electrons in an atom which determine bonding characteristics of an element (# of electrons in outer shell)

Front 47

chemical bond?

Back 47

the formation of compounds from atoms (ionic, covalent, polar covlent)

Front 48

Describe variation of ionization energies of elements on p table?

Back 48

increases across p table from l to r.
Decreases down p table