Unit 1, Chapter 1

Question 1

What is chemistry

Answer 1

The study of matter (anything that has mass and takes up space), the central connection between the sciences.

Question 2

Emperical Knowledge

Answer 2

Knowledge that comes from investigation and observation

Question 3

Theoretical Knowledge

Answer 3

Knowledge based on ideas, created to explain observations

Question 4

Democratus and the Greek Alchemists

Answer 4

Beleived an atom was indivisable after trying to turn iorn to gold.

Question 5

1803

Answer 5

John Dalton’s solid sphere model theory. An atom is a solid mass that cannot be divided. Those of a given element are identical, and they can be combined to create compounds.

Question 6

Blueberry Muffin-top theory

Answer 6

JJ Thompson in 1904. Positivly charged mass with negative charges scattered throughout.

Question 7

Gold Foil Experiement

Answer 7

1911, Ernest Rutherford’s behive model theory. Particles were shot at gold foil. Some passed through and others were deflected at large angles. Positivly charged mass with negative empty space around it.

Question 8

Neils Bohr

Answer 8

1913, Planetary model. Melted elements formed colours. Atoms have energy levels that the negative charges orbit on.

Question 9

1926

Answer 9

Erwin Shrodinger’s quantem model, Electrons move randomly in their set energy level.

Question 10

Octet Rule

Answer 10

8 valence electrons create a stable outer orbit. The execptions to this rule are hydrogen and helium who follow the duet rule.

Question 11

Representative Elements

Answer 11

Follow the rules, rows 1A to 8A

Question 12

Isotopes

Answer 12

atoms of the same element with different numbers of neutrons.

Question 13

Calculating AAM

Answer 13

(mass of isotope 1 x decimal abundance) + all other isotopes in format

Question 14

Radioisotopes

Answer 14

Elements that decay and emit nuclear radiation

Question 15

Alpha particles

Answer 15

largest and least damaging radiation. Same form as helium 4

Question 16

Beta particles

Answer 16

negative electron.

Question 17

Gamma rays

Answer 17

smallest, most damaging

Question 18

Nuclear decay equation

Answer 18

U-235 -> Th-231 + He-4

Question 19

Atomic Radius

Answer 19

distance from nucleus to outermost electrons

Question 20

Ionic Radius in cations

Answer 20

smaller than its atom

Question 21

Ionic radius in anions

Answer 21

larger than its atom

Question 22

Ionization Energy

Answer 22

energy needed to remove an electron. As attraction increases, more energy is needed.

Question 23

Electron Affinity

Answer 23

Energy released with an electron is gained. Greater force of attraction means more energy

Question 24

Electronegativity

Answer 24

the ability of an atom to attract an electron on a scale of 1-4. Greater force of attraction increases electronegativity.

Question 25

What trends go up and across the periodic table

Answer 25

Ionization energy, electron affinity, electronegativity.