Title: Theory / Unimportant / Experimental / Chemistry / Introduction to general organic and biological
Tags: examplesSwitchExample1 hasSeenConjDef defToConstant récupéré

Name: Qualitative test
Definition: Whether something is present or absent
Page: 1

Name: Quantitative test
Definition: How much of something is present
Page: 1

Name: Forensic scientist
Definition: Scientist who identifies the presence or absence of specific chemicals within the body to help solve the criminal case
Page: 1

Name: Chemistry
Definition: study of the composition, structure, properties, and reactions of matter.
Page: 2
Chapter: 1
Example: cook food, add bleach to your laundry, or start your car

Name: Matter
Definition: Anything that make up our world
Page: 2, 58
Chapter: 1, 3
Section: 1, 1

Name: Chemical
Definition: a substance that always has the same composition and properties wherever it is found
Page: 3
Chapter: 1

Question: «Substance» can be used as a substitute word for
Answer: chemical, if it is something precise, matter otherwise
Page: 2, 3
Chapter: 1

Last name: Pauling
First name: Linus
Honor: nobel in peace and chemistry

Name: Scientific method
Definition: Observation: ask questions about what you observe
Page: 4, 5
Chapter: 1
Section: 2
Definition2: Hypothesis: stated in such a way that it can be tested by experiments.
Example: If you sneeze at your friend's house, and they have a cat. try to see whether other cat make you sneeze. Or other thing your friend have
Conjdef: in this order
Definition3: Experiments: several, to test last step.
Definition4: Conclusion: whether second step was true or false in third step

Question: Math part is
Answer: omitted
Page: 6-22
Chapter: 1
Section: 3-4

Question: SI is
Answer: partially omitted
Page: 24
Chapter: 2
Section: 1

Name: Mass of o
Definition: quantity of material o contains
Page: 26
Chapter: 2
Section: 1
Variables: o an object
Typ: kg

Name: Weight of o
Definition: Gravitational pull on o
Page: 26
Chapter: 2
Section: 1
Variables: o an object
Typ: lb

Name: Temperature of o
Page: 26
Chapter: 2
Section: 1
Variables: o an object
Typ: Kelvin

Name: Measured number
Definition: the numbers you obtain when you measure a quantity
Page: 28
Chapter: 2

Name: Significant figures
Definition: all the digits including the estimated digit
Page: 28
Chapter: 2
Variables: m a measure
Abbreviation: SF

Question: Why \(300\) and \(3.0\times 10^2\) are different
Answer: In the first case, there are 3 significant figures
Page: 28
Chapter: 2

Name: Exact number
Definition: numbers obtained by counting items
Page: 29
Chapter: 2
Definition2: using a definition that compares two units in the same measuring system
Example: 60 seconds in a minute
Conjdef: either

Question: The number of significant digits of r_1+r_2 is
Answer: \(\min(n_1,n_2)\)
Page: 30
Chapter: 2
Variables: r_1, r_2 two numbers with n_i significant digits.

Question: The number of significant digits of \(r_1\times r_2\) is
Answer: \(\min(n_1,n_2)\)
Page: 30
Chapter: 2
Variables: r_1, r_2 two numbers with n_i significant digits.

Question: The number of significant digits of \(r_1/r_2\) is
Answer: \(\min(n_1,n_2)\)
Page: 32
Chapter: 2
Variables: r_1, r_2 two numbers with n_i significant digits.

Question: Prefix are
Answer: omitted
Page: 33-34
Chapter: 2
Section: 4

Name: Liter
Definition: dm^3
Page: 33-34
Chapter: 2
Section: 4

Name: Density of s
Definition: mass of s / volume of s
Page: 47
Chapter: 2
Section: 7
Variables: s a substance

Smaller0: o float in l
Greater0: l is denser than o
Page: 45
Chapter: 2
Section: 7
Variables: l a liquid
o an object
Smaller to greater: iff

Question: How to measure the volume of o
Answer: Put o into a liquid, measure the difference in height of the liquid, multiply it by the surface of the recipient
Page: 46
Chapter: 2
Section: 7
Variables: o an object

Name: The specific gravity of s
Abbreviation: sp gr
Chapter: 2
Page: 48
Represents: density of s/density of water
Section: 7
Typ: unitless
Extra: s a substance

Question: Density of water at 4°C
Answer: 1.00g/mL
Page: 48
Chapter: 2
Section: 7

Name: hydrometer
Page: 48
Chapter: 2
Section: 7

Name: Pure substance
Definition: element
Page: 58
Chapter: 3
Section: 1
Definition2: conpound
Conjdef: Matter that has a fixed or definite composition. Either

Name: Element
Definition: composed of only one type of material
Page: 58
Chapter: 3
Section: 1
Example: silver, iron, or aluminum
Intuition: simplest type of a pure substance

Name: Atom
Definition: extremely tiny particles composing element
Page: 58
Chapter: 3
Section: 1

Name: Compound
Definition: pure substance, consisting of atoms of two or more elements always chemically combined in the same proportion.
Page: 59
Chapter: 3
Section: 1

Name: Bonds
Definition: What held together atoms in molecules
Page: 59
Chapter: 3
Section: 1
Context: Chemistry

Name: Molecule
Definition: A group of atoms bound together
Page: 59
Chapter: 3
Section: 1
Example: Water H_2O

Name: Water
Definition: H_2O
Page: 59
Chapter: 3
Section: 1

Name: Hydrogen peroxide
Definition: H_2O_2
Page: 59
Chapter: 3
Section: 1
French: Eau oxygéné

Question: Which of compound, element and mixture can be broken
Answer: compound and mixture, not element
Page: 59
Chapter: 3
Section: 1

Question: How can compound substance be broken
Answer: by chemical reaction only, not physical one
Page: 59
Chapter: 3
Section: 1

Name: Mixture
Definition: two or more different substances which are physically mixed, but not chemically combined.
Page: 59
Chapter: 3
Section: 1
Example: pasta with water
Example2: Steel

Question: How can mixture be broken
Answer: using physical process
Page: 59
Chapter: 3
Section: 1

Name: Homogeneous mixture
Definition: A mixture which is uniform throughout the sample
Page: 59
Chapter: 3
Section: 1
Context: Chemistry
Example: Air
Name2: A solution

Name: Heterogeneous mixture
Definition: A mixture which does not have uniform composition
Page: 59
Chapter: 3
Section: 1
Example: mixture of oil and water

Name: Filtration
Definition: pouring a mixture through a filter paper set in a funnel.
Page: 60
Chapter: 3
Section: 1

Name: Chromatography
Definition: Putting a paper in liquid, letting different liquid move at different pace
Page: 60
Chapter: 3
Section: 1

Question: How to separate solid from liquid
Answer: filtration
Page: 60
Chapter: 3
Section: 1

Question: How to separate different liquid (to know which one are present, not to obtain pure separated liquid)
Answer: Chromatography
Page: 60
Chapter: 3
Section: 1

Name: States of matter
Definition: solid
Page: 62
Chapter: 3
Section: 2
Definition2: liquids
Conjdef: All of
Definition3: gazes
Intuition: The list of physical forms

Name: A solid
Definition: definite shape
Page: 62
Chapter: 3
Section: 2
Definition2: definite volume
Example: Ice, salt, iron
Conjdef: An object with
Definition3: fixed arrangement of particules
Definition4: very strong interaction between particular
Definition5: very slow movement of particles

Name: A gas
Definition: takes shape of the container
Page: 62
Chapter: 3
Section: 2
Definition2: take volume of the container
Example: Water vapor, helium, air
Conjdef: An object wich
Definition3: random/far apart arragement of particles
Definition4: essentially no interaction between particular
Definition5: very fast movement of particles

Name: A liquid
Definition: takes shape of the container
Page: 62
Chapter: 3
Section: 2
Definition2: definite volume
Example: water, oil, vinegar
Conjdef: An object wich
Definition3: random/close arragement of particles
Definition4: strong interaction between particular
Definition5: moderate movement of particles

Name: Physical property
Definition: Property whose characteristics can be observed or measured without affecting the identity of a substance.
Page: 62
Chapter: 3
Section: 2
Example: shape, color, melting point, boiling point, and physical state of a substance

Name: Physical change
Definition: A change of physical state (solid, liquid or gas) without change of the composition
Page: 62
Chapter: 3
Section: 2

Name: Chemical properties
Definition: Property which describe the ability of a substance to change into a new substance.
Page: 63
Chapter: 3
Section: 2

Name: Chemical change
Definition: conversion of some substance into some other substances
Page: 63
Chapter: 3
Section: 2

Name: hypertermia
Definition: Having a temperature at least 3.5°C upper than usual
Page: 67
Chapter: 3

Name: hypotermia
Definition: Having a temperature at least 3.5°C lower than usual
Page: 67
Chapter: 3

Name: Energy
Definition: ability to do work
Page: 68
Chapter: 3
Section: 4
Typ: Joule

Name: Heat
Definition: energy associated with the motion of particles
Page: 68
Chapter: 3
Section: 4

Question: Why does an ice cube feels cold ?
Answer: Heat flows from your hand into the ice cube
Page: 68
Chapter: 3
Section: 4

Question: At which temperature water weight 1.00g/mL?
Answer: 4°C
Page: 48
Chapter: 2
Section: 7