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General Chemistry > Periodic Table > Flashcards

Periodic Table Flashcards

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1
Q

appear in nature in pure form noble gases, carbon, nitrogen, oxygen, gold, silver, and copper

A

Native elements

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2
Q

The _____, alone or in combinations, make up our bodies, our world, our sun, and in fact, the entire universe

A

Elements

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3
Q

Organizes the elements in a particular way that helps one obtain basic information about each of the 118 known elements

A

Periodic Table of Elements

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4
Q

Elements are organized on the table according to their _______, usually found near the top of the square.

A

Atomic number

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5
Q

the “weight” of the atom

A

Atomic mass

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6
Q

Obtained by adding the number of its protons and the number of its neutrons

A

Atomic mass

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7
Q

Some atoms have more or less neutrons than protons. These are called _____?

A

Isotopes

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8
Q

All elements have their own unique symbol. It can consist of a single capital letter, or a capital letter and one or two lower case letters

A

Symbols

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9
Q 
The electrons in the outer energy level of an atom
The electrons (e-) that are transferred or shared when atoms bond together
A

Valence Electrons

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10
Q

What are the Properties of Metal?

A
  • conductor of heat and electricity
  • shiny
  • Ductile
  • Malleable
  • A chemical property of metal is its reactivity with water which results in corrosion
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11
Q

Properties of Nonmetals

A
  • Poor conductors of heat and electricity
  • Neither ductile nor malleable
  • Solid nonmetals are brittle and break easily
  • Dull appearance
  • Many non-metals are gases
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12
Q

Properties of Metalloids

A
  • have properties of both metals and nonmetals
  • solids that can be shiny or dull
  • conduct heat and electricity better than nonmetals but not as efficient as metals
  • ductile and malleable
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13
Q
  • Each columns of elements - group or family
  • Elements in each family have similar but not identical properties.
  • Example - lithium (Li), sodium (Na), potassium (K), and other members of family IA are all soft, white, shiny metals.
  • All elements in a family have the same number of valence electrons.
  • Each horizontal row of elements - period
  • The elements in a period are not alike in properties.
  • Properties change greatly across in a given row.
  • The first element in a period is always an extremely active solid.
  • The last element in a period is always an inert or an inactive gas.
A

Families and Periods

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14
Q
  • sits atop Family AI, but not a member of that family
  • ____ is in a class of its own
  • a gas at room temperature
  • has 1 proton and 1 electron in its 1 and only energy level
  • only needs 2 electrons to fill up its valence shell.
A

Hydrogen

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15
Q
  • Lithium, sodium, and potassium
  • have 1 electron in the valence shell, that is why they are found in group 1
  • all are metals
  • react with group 7 to form metal halides.
A

Group 1

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16
Q
  • The ___ family is found in the 1st column of the periodic table.
  • Atoms of the alkali metals have a single electron in their outermost level - 1 valence electron.
  • They are shiny, have the consistency of clay, and are easily cut with a knife.
  • the most reactive metals
  • react violently with water
  • are never found as free elements in nature
  • are always bonded with another element
A

Alkali Metals

17
Q

What does it mean to be reactive?

A
  • reactive elements bond easily with other elements to make compounds
  • some elements are only found in nature bonded with other elements
18
Q

What makes an element reactive?

A
  • An incomplete valence electron level
  • Octet Rule: All atoms (except hydrogen) want to have 8 electrons in their outermost energy level.
  • Atoms bond until it completes its valence shell with 8 electrons and becomes stable.
  • Atoms with few valence electrons lose them during bonding. Atoms with 6, 7, or 8 valence electrons gain electrons during bonding.
19
Q
  • They are never found uncombined in nature.
  • They have two valence electrons.
  • ______ include magnesium and calcium, among others.
A

Alkaline Earth Metals

20
Q
  • Transition Elements include those elements in the B families.
  • These are the metals you are probably most familiar with: copper, tin, zinc, iron, nickel, gold, and silver.
  • They are good conductors of heat and electricity
  • The compounds of transition metals are usually brightly colored - often used to color paints
  • Transition elements have 1 or 2 valence electrons, which they lose when they form bonds with other atoms. Some transition elements can lose electrons in their next-to-outermost level.
A

Transition Metals

21
Q
  • have properties similar to one another and to other metals, but their properties do not fit in with those of any other family
  • many transition metals combine chemically with oxygen to form compounds called oxides
A

Transition Elements

22
Q
  • named after the first element in the family
  • atoms have 3 valence electrons
  • includes a metalloid (boron), and the rest are metals
  • includes the most abundant metal in the earth’s crust - aluminum
A

Boron Family

23
Q
  • Atoms of this family have 4 valence electrons.
  • includes a nonmetal (carbon), metalloids, and metals
  • The element carbon is called the “basis of life.” Organic Chemistry - an entire branch of chemistry devoted to carbon compounds
A

Carbon Family

24
Q
  • named after the element that makes up 78% of our atmosphere
  • nonmetals, metalloids, and metals
  • have 5 valence electrons
  • tend to share electrons when they bond
  • Other elements - phosphorus, arsenic, antimony, and bismuth
A

Nitrogen Family

25
Q
  • Atoms have 6 valence e-
  • Most elements of this family share e- when forming compounds
  • Oxygen - most abundant element in the earth’s crust, extremely active and combines with almost all elements
A

Oxygen family

26
Q

The element ___ is called the “basis of life.”

A

Carbon

27
Q

most abundant element in the earth’s crust, extremely active and combines with almost all elements

A

Oxygen

28
Q
  • fluorine, chlorine, bromine, iodine, and astatine
  • have 7 valence electrons - the most active nonmetals
  • only need 1 e- to fill their outermost energy level
  • are never found free in nature
  • react with alkali metals to form salts
  • have 7 e- in their outer shell, so they’re found in group 7 of the PT
  • are all colored
  • form metal halides with group 1 metals
  • Fluorine, Chlorine, Iodine - highly effective component of disinfectants and antiseptics
  • Bromine – pesticide
  • Silver bromide is used in photography
A

Halogen Family

29
Q
  • colorless gases that are extremely inert
  • have full outer shells
  • found in group 8 of the periodic table
  • helium, neon, argon, krypton, xenon, and radon.
  • One important property of the noble gases is their inactivity. They are inactive because their outermost energy level is full.
  • Because they do not readily combine with other elements to form compounds, the noble gases are called inert.
  • All the noble gases are found in small amounts in the earth’s atmosphere.
A

The Noble Gases

30
Q
  • The thirty rare earth elements are composed of the lanthanide and actinide series.
  • One element of the lanthanide series and most of the elements in the actinide series are called trans-uranium, which means synthetic or man-made.
  • In 1869, Dmitri Ivanovitch Mendeléev created the first accepted version of the periodic table.
  • grouped elements according to their atomic mass, and as he did, he found that the families had similar chemical properties
  • Blank spaces were left open to add the new elements he predicted would occur.
A

Rare Earth Elements

31
Q

What are the 4 recent discovered elements?

A
  1. Nihonium (Nh) for Element 113
  2. Moscovium (Mc) for Element 115
  3. Tennessine (Ts) for Element 117
  4. Oganesson (Og) for Element 118
32
Q

Is the distance from the nucleus of the atom to the outermost energy level (valence electron)

A

Atomic radius

33
Q

The ease of an atom to lose an electron

A

Metallic property

34
Q

The energy needed by an atom to lose an electron

A

Ionization Energy

35
Q

The ability of the atom to attract an electron to itself

A

Electronegativity

36
Q

The energy released by the atom when it accepts an electron

A

Electron Affinity

General Chemistry (6 decks)

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