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Chem > Chem - Basics > Flashcards

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
Q

Alkaline Earth Metals

A

Group 2 or IIA

26
Q

Transition Metals

A

Groups 3-12 or B groups

27
Q

Halogens

A

Salt makers, group 17 or VIIA

28
Q

Noble/Inert Gases

A

Full valence shell, stable, group 18 or VIIIA

29
Q

Metals

A

Left of staircase; high heat and conductivity, malleable, ductile, lustrous, mostly solids

30
Q

Nonmetals

A

Right of staircase; poor conductors, mostly gases

31
Q

Metalloids

A

Border staircase; intermediate properties

32
Q

Periodic Law

A

When elements are arranged by increasing atomic number properties will repeat and form patterns

33
Q

Atomic size trend (periodic table)

A

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
Q

Electron shielding

A

Core electrons block the nuclear charge over outer electrons

35
Q

Electron shielding trend (periodic table)

A

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
Q

Ionization energy (IE)

A

The amount of energy required for the complete removal of an electron from an atom or ion

37
Q

Ionization energy trend (periodic table)

A

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
Q

Successive Ionization Energy

A

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
Q

Cation

A

Loss of electron; positive charge, smaller atomic size

40
Q

Anion

A

Addition of electron; negative charge, larger atomic size due to dilution of positive charge

41
Q

Electronegativity

A

Ability of an atom in a covalent bond to attract the shared electron pair

42
Q

Polar covalent bond

A

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
Q

Electronegativity trend (periodic table)

A

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

Chem (10 decks)

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