Chem - Basics Flashcards

1
Q

Matter

A

Both has mass and takes up space (volume)

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2
Q

Mass

A

How much matter

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3
Q

Weight

A

How much force

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4
Q

Substance

A

Matter of uniform and defined composition, made up of only 1 kind of matter

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5
Q

Element

A

A substance that cannot be broken down into simpler substances, simplest type of substance with unique properties

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6
Q

Law of definite proportions

A

A compound contains the same elements in the same proportions regardless of sample size and source

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7
Q

Empirical Formula

A

Lowest whole number of moles, gives relative number of atoms of each element in a compound

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8
Q

Molecular formula

A

Actual number of atoms of each element in a compound

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9
Q

Structural formula

A

Shows placement and connections of atoms in a molecule

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10
Q

Physical properties

A

Properties shown by the substance itself, without interactions with another substance

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11
Q

Chemical properties

A

Properties shown by a substance when it interacts with or transforms into other substances

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12
Q

Law of conservation of mass

A

Matter can neither be created nor destroyed

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13
Q

Solution

A

A homogeneous mixture of multiple substances

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14
Q

Miscible

A

A substance that is infinitely soluble in another substance

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15
Q

Dalton’s Atomic Theory

A

All matter is composed of atoms; atoms of one element are identical to each other and different than atoms of another element; atoms can only change when combined with other elements

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16
Q

Atomic number (Z)

A

Characteristic number of protons in the nucleus of atoms of a particular element, identifies element

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17
Q

N number (N)

A

Number of neutrons in the nucleus of an atom, identifies isotopes

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18
Q

Mass number (A)

A

Number of protons and neutrons in the nucleus of an atom, identifies mass

19
Q

Isotope

A

An atom of an element with the same number protons but a different number of neutrons

20
Q

Atomic Mass Unit (AMU)

A

A unit of mass equal to 1/12 the mass of a carbon-12 atom

21
Q

Ion

A

An atom or group of atoms that has a positive or negative charge

22
Q

Molarity (M)

A

Concentration of solute in a solution, M = n/L (molarity = moles solute/litres of solution)

23
Q

Valence Electrons

A

Electrons involved in bond formation, typically held in the outermoat shell

24
Q

Alkali metals

A

Basic in water, group 1 or IA

25
Alkaline Earth Metals
Group 2 or IIA
26
Transition Metals
Groups 3-12 or B groups
27
Halogens
Salt makers, group 17 or VIIA
28
Noble/Inert Gases
Full valence shell, stable, group 18 or VIIIA
29
Metals
Left of staircase; high heat and conductivity, malleable, ductile, lustrous, mostly solids
30
Nonmetals
Right of staircase; poor conductors, mostly gases
31
Metalloids
Border staircase; intermediate properties
32
Periodic Law
When elements are arranged by increasing atomic number properties will repeat and form patterns
33
Atomic size trend (periodic table)
Decreases across a period due to added protons having a stronger pull on the valence shell; increases down a group as additional shells are formed
34
Electron shielding
Core electrons block the nuclear charge over outer electrons
35
Electron shielding trend (periodic table)
Stays constant across a period due to containing the same number of core electrons; increases down a group as more core shells are added
36
Ionization energy (IE)
The amount of energy required for the complete removal of an electron from an atom or ion
37
Ionization energy trend (periodic table)
Increases across a period due to the stronger pull of protons on electrons; decreases down a group due to electrons being further from the nucleus and therefore shielded from proton attraction
38
Successive Ionization Energy
Energy required to remove successive electrons; increases with each electron due to increased positive charge, massive increase when full outer shell is removed and the new outer shell is complete
39
Cation
Loss of electron; positive charge, smaller atomic size
40
Anion
Addition of electron; negative charge, larger atomic size due to dilution of positive charge
41
Electronegativity
Ability of an atom in a covalent bond to attract the shared electron pair
42
Polar covalent bond
A bond in which the electron pair is not shared equally due to differences in electronegativity, causes the molecule to have partially charged regions
43
Electronegativity trend (periodic table)
Increases across period due to stronger positive force of protons on electrons; decreases down a group due to weaker positive force of protons on electrons