General Chemistry 1 Final Ualbany

Front 1

Celsius to Farenheit

Back 1

9/5(C) + 32

Front 2

Farenheit to Celsius

Back 2

5/9(F − 32)

Front 3

Density equals

Back 3

mass/volume

Front 4

Rules for Significant Figures

Back 4

All nonzero digits are significant.

Zeroes between two significant figures are themselves significant.

Zeroes at the beginning of a number are never significant.

Zeroes at the end of a number are significant if a decimal point is written in the number.

Front 5

Accuracy

Back 5

the proximity of a measurement to the true value of a quantity

Front 6

Precision

Back 6

refers to the proximity of several measurements to each other

Front 7

One inch to cm

Back 7

1 inch = 2.54cm

Front 8

AMU = __ grams

Back 8

1 amu =1.66054 × 10-24 g

Front 9

Scientist and tool credited with discovery of electrons

Back 9

J. J. Thompson

cathode tubes

Front 10

Charge/Mass ratio of electron

Back 10

1.76  108 coulombs/g

Front 11

Discovered the charge of electron in 1906 at UChicago

Back 11

Robert Millikan (University of Chicago) determined the charge on the electron in 1909

Front 12

First observed radiation

Back 12

Henri Becquerel

Front 13

alpha particles

Back 13

two protons
two neutrons

discovered by Ernest Rutherford

Front 14

Beta- Particle

Back 14

An emitted electron

Discovered by Ernest Rutherford

Front 15

Beta+ particle

Back 15

Positron

Discovered by Ernest Rutherford

Front 16

Gamma radiation/particles

Back 16

very fast electromagnetic radiation of subatomic particles

Front 17

Dimensions of atoms measured by

Back 17

1 Å =10-10 m

Front 18

mass spectrometer

Back 18

measures atomic weights

Front 19

Name of group 6A

Back 19

Chalcogens

Front 20

Metalloids

Back 20

B
Si
Ge As
Sb Te

Front 21

The Diatomic Molecules

Back 21

H ave
N o
F ear
O f
I ce
Cl cool
B eer

Front 22

Aluminum takes a ___ charge

Back 22

Al 3+

Front 23

Nitrogen takes a ___ charge

Back 23

N 3-

Front 24

Chalcogens takes a ___ charge

Back 24

Chalcogens: 2-

Front 25

Zinc takes on a ___ ion

Back 25

Zn 2+

Front 26

Calcium takes on a __ charge

Back 26

Calcium: 2--

Front 27

% element
or
% composition

Back 27

(#atoms)(#atomic weight)
_____________________
(Formula Weight of compound)

all times 100

Front 28

Avogadro's Number

Back 28

6.02*10^23

Front 29

An 18g laboratory-sized sample of water contains ____

Back 29

18g = 1 mole of H2O

Front 30

% Yield

Back 30

(Actual/Theoretical) *100

Front 31

solutions

Back 31

homogeneous mixtures of two or more pure substances

Front 32

solvent

Back 32

greatest abundance

Front 33

Solutes

Back 33

smaller

Front 34

dissociation

Back 34

When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them.

Front 35

electrolyte

Back 35

An electrolyte is a substances that dissociates into ions when dissolved in water.

Front 36

Strong Acids

Back 36

HCl, HBr, HI, HClO3, HClO4, HNO3, H2SO4

Front 37

Strong bases

Back 37

Alkali-OH, Ca, Sr, Ba-OH

Front 38

Steps to writing net ionic equations

Back 38

Write a balanced molecular equation.

Dissociate all strong electrolytes.

Cross out anything that remains unchanged from the left side to the right side of the equation.

Write the net ionic equation with the species that remain.

Front 39

Net ionic equation of strong neutralization reactions

Back 39

H+ + OH- ==> H2O

Front 40

Oxidation Rules

Back 40

Oxygen has an oxidation number of −2, except in the peroxide ion in which it has an oxidation number of −1.

Hydrogen is −1 when bonded to a metal, +1 when bonded to a nonmetal.

Fluorine always has an oxidation number of −1.

The other halogens have an oxidation number of −1 when they are negative; they can have positive oxidation numbers, however, most notably in oxyanions.

Front 41

displacement reactions

Back 41

ions oxidize an element.

Front 42

Kinetic Energy equation

Back 42

KE = 1/2 mv^2

(one-half mass velocity squared)

Front 43

1 cal = ____ J

Back 43

1 cal = 4.184 J

Front 44

work = ___ x ___

Back 44

Work = force x distance

Front 45

First Law of Thermodynamics

Back 45

Energy is neither created nor destroyed

Front 46

Internal Energy

Back 46

Potential and kinetic energies all summed up

Front 47

Heat equation

Back 47

Final temp - Initial temperature

Front 48

Endergonic

Back 48

Absorbs energy from surroundings

Front 49

Exergonic

Back 49

Releases energy into surroundings

Front 50

Internal Energy:

State function or not?

Back 50

Initial Energy IS a state function

q and w are NOT

Front 51

work done by gas = __ ___

Back 51

work = -P /\ V

Front 52

Enthalpy (Heat) =

Back 52

H = E +PV

Front 53

If /\H is positive

Back 53

Endothermic

/\H=+

Front 54

If a process has a negative /\H

Back 54

It's exothermic

Front 55

Enthalpy /\H

Back 55

total /\H = /\H products - /\H reactants

Front 56

Enthalpy is an ____ property

Back 56

extensive

Front 57

Hess' Law

Back 57

If a reaction is carried out in a series of steps, /\H for the overall reaction will be equal to the sum of enthalpy changes for the individual steps

Front 58

/\ H = (Hess' Law)

Back 58

/\H = total products - total reactants