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Chemistry > unit 4 > Flashcards

unit 4 Flashcards

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1
Q

Alkali metal

A

An element in Group 1 of the periodic table. These elements are extremely reactive and will react spontaneously with water creating hydrogen gas and hydroxide ions in solution.

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2
Q

Alkaline Earth Metal

A

An element in Group 2 of the periodic table. These elements are reactive (but less so than Group 1), creating hydrogen gas and hydroxide ions in solution.

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3
Q

Anion

A

A negatively charged ion

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4
Q

Atomic radius

A

Half the distance between adjacent nuclei. Size of an atom in Picometers (pm)

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5
Q

Brittle

A

The ability to be crushed into pieces when hammered, a property of nonmetals.

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6
Q

Cation

A

A positively charged ion.

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7
Q

Diatomic Molecule

A

A nonmetal atom that forms one or more nonpolar covalent bonds with another atom of the same element to form a molecule consisting of the two atoms when there is no other element to bond with. Elements that do this are Br, I, N, Cl, H, O and F. BRINClHOF like brinklehoff

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8
Q

Ductile

A

The ability to be stretched into a wire, a property of metals.

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9
Q

Dull

A

The lack of ability to reflect light efficiently, a property of nonmetals.

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10
Q

Group

A

Columns down the periodic table that contain elements with the same number of valence electrons and thus similar chemical properties. Aka “families”

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11
Q

Electronegativity

A

The relative ability for an atom to gain an electron. Fluorine has the highest electronegativity 4.0. INCREASES across a period and DECREASES down a group

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12
Q

Effective nuclear charge

A

The overall attraction to the nucleus that a valence electron experiences. This increases as the # of protons increases and the occupied number of energy levels remains the same

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13
Q

Halogen

A

An element in Group 17 of the periodic table. These elements are extremely reactive, not as much as groups 1 and 2. e.g. fluorine, chloride, bromine, etc

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14
Q

Ionization energy

A

The energy required to remove an electron from the valence shell. Unit: kJ/mol Kilojoules per mol. It INCREASES across a period and DECREASES down a group.

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15
Q

Ionic radius

A

The size of an ion compared to the original atom. Metal atoms lose electrons and form + charged ions that are SMALLER than the original atom, nonmetal atoms form – charged ions that are LARGER than the original atom.

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16
Q

Luster

A

The ability to reflect light, a property of metals.

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17
Q

Malleable

A

The ability to be hammered or rolled into thin sheets, a property of metals.

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18
Q

Metal

A

Elements that have low electronegativity and ionization energy and large radius that tend to lose electrons to form chemical bonds. Most of the periodic table is metals

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19
Q

Metallic Character

A

describes the set of chemical properties that are usually associated with the elements classified as metals in the periodic table ie. LOSING ELECTRONS conductor, malleable, ductile. increases <- and v

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20
Q

Metalloid

A

Elements that exhibit properties of both metals and nonmetals. B, Si, Ge, As, Sb, Te (sometimes Po and As)

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21
Q

Orbital

A

The location in the electron cloud with the highest probability of finding an electron.

22
Q

Monatomic atom

A

A molecule composed of just one atom

23
Q

Noble gases

A

A Group 18 element on the periodic table. These elements are nonreactive, with a full valence shell (8).

24
Q

Nonmetal

A

Elements that have high electronegativity and ionization energy and small radius that tend to gain or share electrons to form chemical bonds.

25
Q

Properties of metals

A

good conductors of heat and electricity, dense, malleable, ductile, lose electrons easily, high melting points, lustrous, solid at room temp (EXCEPT MERCURY)

26
Q

Properties of non metals

A

bad conductors of heat and electricity, low density, brittle, gains electrons easily, low melting points, dull.

27
Q

Properties of metalloids

A

variable conductors of heat and electricity, variable density, brittle, gains or loses electrons, variable melting points, and lustrous.

28
Q

Nonreactive

A

Not capable of readily gaining or losing e’s or undergoing a chemical change/reaction. INERT. e.g. noble gases

29
Q

Oxidation

A

The loss of valence electrons from an atom or ion, resulting in the increase in oxidation number of an element.

30
Q

Periodic law

A

Properties of elements repeat in a predictable way when arranged by atomic number

31
Q

Periods

A

Rows across the periodic table with elements having the same number of occupied principal energy levels.

32
Q

Rare Earths/Inner Transition metals

A

F Block elements. Fill the F orbitals. Many are radioactive.

33
Q

Reactivity

A

aka “activity” is a measure of how readily a substance undergoes a chemical reaction.

34
Q

Reduction

A

The gain of valence electrons from an atom or ion, resulting in the decrease in oxidation number of an element.

35
Q

shielding effect

A

a decrease in attraction between electrons and the nucleus in an atom due to distance and repulsion between extra electrons and energy levels between the nucleus and valence electrons. More internal or “core electrons” lesson the effect of the nucleus on valence electrons

36
Q

shielding electrons

A

non-valence electrons, AKA core electrons

37
Q

transition metals

A

Metals from D Block. Display classic metallic properties. Hard, shiny, ductile, malleable and they make COLORED IONS in solution and colored crystals as a solid. They also have multiple oxidation numbers (polyvalent)

38
Q

Z effective

A

The net attraction from the positive nucleus that a negative valence electron can “feel”. The core electrons are said to shield the valence electrons from the full attractive forces of the protons in the nucleus.
Zeff = Z -S Z is nuclear charge, S is the number of core electrons. The higher the Zeff, the greater the relative attraction for valence electrons

39
Q

Antoine Lavoisier

A

“Father of modern chemistry” who first organized the ‘elements’ (some were compounds, not elements). His ‘list of simple substances’ was ordered based off of reactivity w/ oxygen and other elements

40
Q

Johann Dobereiner

A

scientist who made Model of Triads in 1829. He grouped 3 sets of 3 elements with similar chemical properties (e.g. Li, Na, and K reacting with water, chlorine and hydrogen similarly).

41
Q

Law of triads

A

Law connected to Johann Dobereiner which states the atomic mass of the middle element in a triad about equals the mean of the 1st and 3rd atomic masses. (1st observed pattern in the elements)

42
Q

John Newlands

A

Scientist who created the law of octaves in 1865.

43
Q

Law of Octaves

A

law created by John Newlands. When elements placed in order of atomic weights, every 8th element has similar properties to the 1st. (predecessor of periodic law)

44
Q

Dmitri Mendeleev

A

OUR MAN who created 1st periodic table in 1869. He arranged them in a grid and listed elements in atomic mass. He predicted the existence and properties of elements not yet discovered e.g. Gallium

45
Q

Henry Moseley

A

Made the modern periodic table! He ordered the elements in increasing atomic number.

46
Q

Moseley’s experiments

A

Lowkey don’t understand this ahaha
Moseley shot beta particles at atoms and on impact, each element emitted an X ray with a unique frequency. He made graph by plotting the sq root of the x ray frequency vs the atomic number, and found that it was an increasing linear graph. This means that the atomic number was equal to the amount of charge in the nucleus, and the atomic number = the number of protons

47
Q

Periodicity

A

tendency to recur at intervals

48
Q

How to know valence electrons based on spdf notation

A

total number of s and p in the highest PEL

49
Q

Alloy

A

mixture or blend of 2 or more metallic elements. Made from melting then mixing metals, properties differ to original metals.

50
Q

representative elements

A

elements group 1,2,13-18 that make up the ‘main group’ of elements with regular properties i think

Chemistry (18 decks)

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