Chapter 2 And 1.3 Flashcards

(28 cards)

0
Q

Element vs. compound

A

Element: substance made form ONLY one type of atom

Compounds: substances made form 2 or more types o atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
1
Q

Pure substance vs. mixture

A

Pure substance: all particles are the same and no & defined an constant

Mixture: different particle types
A combination of pure substances

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Physical properties vs. chemical properties

A

Physical: can be observed without changing identity of substance

Chemical: can only be observed when substances react with something else

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Physical change vs. chemical change

A

Physical: a change in appearance, but no change in composition

Chemical: a new substance is formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Extensive vs. intensive properties

A

Extensive: depends on substance amount ( mass and volume)

Intensive: does not depend on amount of substance. (Color, smell)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Solids vs. liquids vs. gases

A

Solid: independent shape, tight particles, has shape and volume.
Liquid: close particles, not independent shape
Gas: fills volume (expands), far apart particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Reactants vs. products

A

Reactant: chronicles present at start of reaction

Product: chronicles produced in reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Exothermic vs. endothermic reactions

A

Exothermic: give off heat

Endothermic: absorbed heat

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Four indications of chemical reaction

A
  1. Transfer in energy (heat/light)
  2. Change in color
  3. Production of gas
  4. Formation of precipitate
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Defiance precipitate

A

A solid that forms and settles on the bottom of an aqueous solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does the law of conservation of mass state

A

In a physical and chemical change always stays the SAME

Product weight= reactant weight

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Reversible vs. irreversible change

A

Reversible: melting and freezing

Irreversible: tearing paper

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Matter

A

Everything with mass and volumes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the difference between an Observation and an Inference

A

Observation- information gathered using the 5 senses and measurement

Inference- conclusion based on the observations and past knowledge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Define chemistry

A

The study of matter and it’s changes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Lab safety

A

Freakin common sense

16
Q

Measuring to the correct decimal

A

Measure to what you can and guess once

17
Q

Define an atom

A

Atom is smallest particle of an element that retains its identity in a chemical reaction

18
Q

View of an atom changes overtime

A
  1. Democritus
    Thought atoms were solid spheres (smallest they get)
  2. Dalton
    Tough matter consisted of small lumps (atoms)
  3. Thomson
    Plumb pudding model (discovered electron and thought it would also have something positively charged)
  4. Goldstein
    He discovers the nucleus
5. Ruthoford
    Electron cloud through tin foil experiment. 
6. Bohr
     Electron orbitals
7. Chadwick
     Discovered the neutron
19
Q

Compare and contrast subatomic particles (electron, proton, neutrons)

A

Electron e- -1 charge 1/1849 mass 9.11x10 to the -28th mass

Proton p+ +1 charge 1 mass 1.67x10 to the -24th mass

Neutron n0 0 charge. 1 mass 1.67x10 to the -24th mass

20
Q

Interpret a nuclear symbol

A

Mass # is the top left
Atomic # is the bottom left
Charge is the top right

Mass - atomic number = neutrons

21
Q

Isotope

A

Atoms with different number of neutrons

22
Q

Define average atomic mass and how to calculate it

A

It’s the weight average of all the naturally occurring isotopes in that element. Found on periodic table below element symbol.

23
Q

Describe how the Bohr of an atom improved upon earlier models.

A

It specified that electrons ain’t in electron clouds but in specific paths (orbits) around the nucleus. The highest energy
Level is furthest from the nucleus.

24
Difference between quantum mechanical model and previous atom models.
This gives you the likeliness of finding an electron in various locations around the nucleus. No longer orbits (circular paths) but now Orbitals (area of location probability)
25
Define orbitals
Areas of location probability.
26
How to write electron configuration (3 rules) See orange tab thing
1. Aufbau Principle Build from the bottom up. 2. Pauli Exclusion (kinda like a magnet) Each orbital may have a max. Of 2 electrons (opposite spins) 3. Hunds Rule (monopoly rule) An electron must be on each property before adding
27
Now how to write a noble gas configuration
Ex [Ne] 2S2