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Chemistry of Solutions > Lecture 1-1 > Flashcards

Lecture 1-1 Flashcards

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1
Q

Matter

A
  • Anything that occupies space and has mass

- Made up of atoms/molecules

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2
Q

Solids

A

Have a fixed shape and mass

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3
Q

Liquids

A
  • Take the shape of their container

- Has fixed volume with horizontal surface

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4
Q

Gas

A

Expand to fill their container

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5
Q

Mixture

A

Physical combination of two or more substance that retain their individual properties
Ex: sugar water

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6
Q

Pure substance

A

Form of matter with constant chemical composition and characteristic properties
Ex: table sugar/sucrose

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7
Q

Compound

A

Pure substance which can be broken down into a simpler substance by a chemical charge

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8
Q

Element

A

Pure substance that cannot be broken down

Primary constituent of matter

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9
Q

Atom

A

Smallest particle of an element.

  • Has properties of its element
  • Can enter chemical combination
  • Composed of protons, neutrons, electrons
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10
Q

Molecule

A

Two or more atoms joined together, linked by chemical bond

- Can be made of the same of different atoms

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11
Q

Ion

A

Atoms with a net ionic charge due to loss or gain of electrons

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12
Q

Electron

A

stable negatively charged component of an atom

- Charge of 1.602x10^-19 coulombs

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13
Q

Molecular compound

A

Pure substance formed by two or more atoms of different non-metals that share a covalent bond
- Linked by sharing electrons

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14
Q

Ionic compound

A

Substance formed by ions linked together by electrostatic forces (ionic bond)

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15
Q

Physical Property

A

Measurable characteristic that does not change the composition of matter
Ex: color, hardness, melting point, boiling point, density

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16
Q

Physical change

A

Change to the physical state, form or properties of matter
- Does not change the chemical composition of the substance
Ex: liquid to solid

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17
Q

Chemical property

A

A property or characteristic observed during a reaction where the identity or chemical composition of the substance is changed
Ex: toxicity, flammability, heat of combustion, acidity

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18
Q

Extensive property

A

Depends on the amount of matter present

- Ex: mass, volume

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19
Q

Intensive property

A

Does not depend on the amount of matter present

Ex: temperature

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20
Q

Describe an atoms makeup

A
  • Small core - nucleus: made of positively charged protons/uncharged neutrons
  • Nucleus surrounded by large volume of space containing negatively charged electrons
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21
Q

Where is most of the atoms mass contained?

A

Nucleus bc protons/neutrons are heavier than electrons

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22
Q

Atomic mass unit

A
  • (1/12 the mass of a carbon atom containing six protons and neutrons)
23
Q

1 amu = ?

A

1 amu = (1.6605x10^-24)g

1 amu = 1 Da (Dalton) = 1 u (unified atomic mass unit)

24
Q

Fundamental unit of charge (e)

A

the magnitude of the charge of an electron e= (1.602 x10^-19)C

25
Q

Atomic number (Z)

A

number of protons

26
Q

Mass number (A)

A

protons+electrons

27
Q

Number neutrons

A

A-Z

mass number-number of protons

28
Q

Neutral atom

A

same number of protons and electrons

29
Q

Ions

A

Atom does not have the same amount of protons and electrons

They are electrically charged

30
Q

Atomic charge

A

protons-electrons

31
Q

Anion

A

Gain electron - negatively charged

32
Q

Cation

A

Lose electron

Postively charged

33
Q

Chemical symbols

A

Abbreviation used to indicate an element of an atom

each element has a unique chemical symbol associated to a unique atomic number

34
Q

Isotope

A 
Atom with the same number protons, but neutrons differ 
Isotopes with a slightly different mass
Ne-20 (10 neutrons)
Ne-21 (11 neutrons)
Ne-12 (12 neutrons)
35
Q

Atomic mass

A

approximately equal to atoms mass number

36
Q

Molecular formula

A

Represents a molecule using chemical symbols and subscripts indicating number of types of each atom

37
Q

Structural formula

A

H-O-H

38
Q

Empirical formula

A

Give the relative number of atoms of each element in the compound (Molecular formula gives the actual number of atoms)

39
Q

Give empirical and molecular formula of H2O2

A

Empirical: HO
Molecular: H2O2

40
Q

Isomers

A

Molecule with the same formula but different structures

41
Q

Learn periodic table column names

A

b

42
Q

Metals characteristics

A

Good conductors of heat and electricity
• Malleable
• Ductile
• Tend to lose electrons when they undergo chemical changes

43
Q

Nonmetals characteristics

A
  • poor conductors
  • tend to gain electrons
  • can be solid, liquid or gas
44
Q

Mettaloids characteristics

A

• have mixed properties
• have intermediate and temperature dependant electrical
conductivity

45
Q

Noble gas characteristics

A

mostly unreactive

46
Q

Alkali Metals

A

Reactive
• Lose one electron from chemical change to have same
number of electrons as nearest noble gas

47
Q

Alkaline earth metals

A

fairly reactive
• lose two electrons from chemical change to have same
number of electrons as nearest noble gas

48
Q

Halogens

A

very reactive non-metals
• gain one electron from chemical change to have same
number of electrons as nearest noble gas

49
Q

Density

A

Ration of mass over volume of a substance at a specific temperature

Units: g/cm3
or g/mL (reminder 1 cm3 = 1 mL)
d=m/V

50
Q

Temperature (K)

A

Kelvin

Conversion: 0 C is equivalent to 273.15 K
K = C + 273.15 K

51
Q

Accuracy

A

How close a measured value is to an actual value

52
Q

Precision

A

How close a series of measurement are to one another and how reproductible they are

53
Q

Teaxt book

A

Chapter 1: 8-92

Chapter 2: 10-19, 27-30

Chemistry of Solutions (2 decks)

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