Terms

Question 1

What is the atomic theory?

Answer 1

• each element is composed of particles called atoms
• all atoms of a given element have the same mass and properties that distinguish them from atoms of other elements
• atoms combine to form compounds
• atoms of one element cannot change into atoms of another element

Question 2

theory

Answer 2

a well tested explanation of why something happens; WHY

Question 3

observations

Answer 3

what you see happens and some physical measurement you can make.

Question 4

law

Answer 4

a concise summary of a large number of observations or experiments; can predict what will happen, but a theory is needed to explain why it happened; WHAT

Question 5

examples of crystalline and amorphous solids

Answer 5

crystalline: arranged molecules like salt and diamonds
amorphous: do not have a well-ordered geometric shape like glass or plastic

Question 6

accuracy

Answer 6

how close the measured value is to the actual value

Question 7

precision

Answer 7

how close a series of measurements are to one another or how reproducible they are

Question 8

systematic error

Answer 8

part of the experiment, predictable, occurs each time you measure. (unreliable scales off a few grams)

Question 9

random error

Answer 9

external source causes problems, no way of predicting, will only occur sometimes (cloud goes over sun and lowers room temp.)

Question 10

Law of Definite Proportions

Answer 10

all compounds, regardless of their sources or how they were prepared, have the same proportions of their constituents

Question 11

nuclear theory

Answer 11

• most of the atom’s mass and positive charges are in the nucleus
• most of the volume is empty space where electrons are dispersed
• electrons and protons are equal so that the atom is electrically neutral

Question 12

an element’s molar mass is numerically equal to…..

Answer 12

the elements atomic mass units (amu)

Question 13

ionic bond

Answer 13

metal + nonmetal

Question 14

covalent/molecular bond

Answer 14

nonmetal + nonmetal

Question 15

acids

Answer 15

behind with H+

Question 16

percent yield

Answer 16

actual/theoretical

Question 17

percent composition

Answer 17

mass of element “x” in one mole of compound/ mass of 1 mole of the compound

Question 18

Boyle’s Law

Answer 18

p1v1=p2v2

Question 19

Charle’s Law

Answer 19

v1/t1=v2/t2

Question 20

Avogadro’s Law

Answer 20

v1/n1=v2/n2

Question 21

ideal vs. real gas

Answer 21

• real gases do not behave like ideal gases at high P or low T.
• ideal gas law assume no attraction between gas molecules ands gas molecules do not take up space (not valid at low T and/or high P

Question 22

kinetic molecular theory

Answer 22

• the size of a particle is very small
• the average kinetic energy of a particle is proportional to the temperature (in K)
• all collisions are elastic

Question 23

energy

Answer 23

the capacity to do work

Question 24

work

Answer 24

the result of a force acting through a distance

Question 25

1st Law of Thermodynamics

Answer 25

- energy cannot be created or destroyed | - total energy of the universe is constant

Question 26

Energy is transferred only by....

Answer 26

work (w) or heat (q)

Question 27

pressure= ______/________

Answer 27

force/area

Question 28

barometer

Answer 28

uses height of a liquid to measure the barometric pressure

Question 29

amplitude

Answer 29

measure of wave intensity

Question 30

wavelength

Answer 30

wavelength or frequency of light waves determines its colour

Question 31

photons

Answer 31

the energy of the particles of light

Question 32

n (quantum mechanics)

Answer 32

principal quantum number | -main energy level (shell)

Question 33

l (quantum mechanics)

Answer 33

angular momentum quantum number | -gives info on shape (s,p,d,f)

Question 34

ml (quantum mechanics)

Answer 34

magnetic quantum number | -specifies orientation of orbital

Question 35

Aufbau Principle

Answer 35

orbitals in the same sub shell have the same energy (degenerate) -place one e- in each before completing pairs

Question 36

Hund's Rule

Answer 36

2 e- in separate orbitals will have lower energy than 2 e- in the same orbital b/c of decreased e- to e- repulsion

Question 37

Pauli Exclusion Principle

Answer 37

no more than 2 e- per orbital

Question 38

paramagnetism

Answer 38

has unpaired e- and will have a net magnetic field

Question 39

diamagnetism

Answer 39

had only paired e- and will have no magnetic field

Question 40

Non-Polar Covalent

Answer 40

- electrons shared equally | - 0-0.4

Question 41

Polar Covalent

Answer 41

- electrons shared unequally | - 0.4-2.0

Question 42

Ionic Bond

Answer 42

- electrons transferred | - 2.0-3.3

Question 43

The _______ the __________________ the higher the vapour pressure.

Answer 43

-weaker, intermolecular forces

Question 44

As temperature increases, the vapour pressure ____________.

Answer 44

increases

Question 45

vaporization is....

Answer 45

endothermic

Question 46

condensation is.....

Answer 46

exothermic