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Gen chem > Periodic > Flashcards

Periodic Flashcards

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1
Q

Arrangement of atoms in various energy levels

A

Electron configuration

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2
Q

Tool used to show the arrangement of elements in an organized manner

A

Periodic table of elements

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3
Q

Elements are arranged in increasing atomic weight.
Has similar physical and chemical properties which occurs after each interval of 7 elements.
Who is the proponent?

A

Law of Octaves by John Newlands

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4
Q

Elements are arranged in increasing atomic mass, in groups if 3 (triads) having similar chemical properties.
Who is the proponent?

A

Law of Triads by Dobereiner

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5
Q

Created his own version of the periodic table listing the most known elements at the time by their increasing atomic mass and who is the proponent.

A

Modern periodic table by Dmitri Mendeleev

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6
Q

His arrangement left gaps, which led to the discovery of elements yet to be discovered.

A

Modern periodic table by Dmitri Mendeleev

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7
Q

Introduced the concept of atomic numbers in the periodic table.

A

Modern periodic table by Henry Moseley

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8
Q

Elements are arranged in increasing atomic number.
Atomic mass is a weighted average of all naturally occurring isotopes.

A

The periodic table

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9
Q

2 useful ways to classify elements

A

The metals, nonmetals, and metalloids and periods and families.

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10
Q

Located on the left side of the periodic table

A

Metals

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11
Q

Are brittle, aren’t malleable and ductile, and poor conductors of heat and electricity.

A

Nonmetals

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12
Q

Tend to gain electrons in a chemical reaction

A

Nonmetals

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13
Q

They are economically important as they have unique conductivity properties which makes them valuable in the semiconductor and computer chip industry

A

Metalloids or semi-metals

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14
Q

Are the horizontal rows in the periodic table and are numbered 1-7 in the left side of the periodic table.

They do not have very similar properties

A

Periods

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15
Q

Are the vertical columns in the periodic table. Older methods used are roman numerals and letters.

They have similar properties

A

Families or groups

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16
Q

Highly reactive with water

A

1A Alkali metals

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17
Q

Reactive with water, and increases as you move down the group

A

2A alkali earth metals

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18
Q

Not as well-known as other elements.
Most known element is Aluminum

A

3A Earth metals/Boron Group

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19
Q

Refers to their ability to carry charge of 4

A

4A Tetrels/Carbon Group

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20
Q

Intermediate between those of metals and nonmetals

A

5A Pnictogens/ Nitrogen Group

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21
Q

changing from nonmetallic to metallic as you move down the family

A

6A Chalcogens/ Oxygen Group

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22
Q

Creates/ Forms salts; high electron affinities

A

7A Halogens

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23
Q

Highly stable, unreactive

A

8A noble gases

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24
Q

D and F block metals with 2 valence electrons

A

3B-12B Transition metals

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25
Q

Specific pattern present in the periodic table which illustrate the different aspects of certain elements including its size and electronic properties

A

Periodic Trends

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26
Q
  1. Moves left to right across the period
  2. Moves top to bottom down a group
A
  1. Electronegativity- increases (period)
  2. Electronegativity- Decreases (groups)
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27
Q
  1. Moves left to right across the period
  2. Moves top to bottom down a group
A
  1. Ionization Energy- increases (period)
  2. Ionization Energy- Decreases (groups)
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28
Q
  1. Moves left to right across the period
  2. Moves top to bottom down a group
A
  1. Electron Affinity- increases (period)
  2. Electron Affinity- Decreases (groups)
29
Q
  1. Moves left to right across the period
  2. Moves top to bottom down a group
A
  1. Atomic Radius- decreases (period)
  2. Atomic Radius- increases (groups)
30
Q
  1. Moves left across the period and down the group
  2. Moves right across the period and up the group
A
  1. Metallic Property- increase metallic character
  2. Metallic Property- decrease metallic character
31
Q

Atoms form compounds to achieve a filled valence energy level. Atoms in some compound share electrons.

A

Covalent bonds

32
Q

Why do atoms have to share?

A

Chemical bond that comes from the sharing of 1 or more electronic pair between 2 atoms

33
Q

3 ways to represent covalent bonds

A

A. Overlapping of electron orbitals, and the sharing of electron pair
B. Electron-dot formula
C. Lewis structural formula

34
Q

Uses complex shape of orbitals

A

Quantum mechanical model of atom

35
Q

Scientists introduced 4 numbers to describe the characteristics of electrons and their orbitals

A

Quantum Numbers

36
Q

What are the 4 quantum numbers

A

Principal (n), Angular Momentum (l), Magnetic (ml), Spin (ms)

37
Q

Defined as atom or groups of atoms within a molecule that has similar chemical properties whenever it appears in various compounds

A

Functional Group

38
Q

Contains 1 or more double bonds between neighboring carbon atoms

A

Alkenes

39
Q

Contains 1 or more triple bonds between neighboring carbon atoms

A

Alkynes

40
Q

Functional group that contains a ring
Contains alternating double bonds

A

Aromatics or Aromatic Ring

41
Q

Large molecules necessary for life and built from smaller organic molecules

A

Biological Molecules

42
Q

4 major classes of biological macromolecules

A

Carbohydrates, lipids, protein, nucleic acid

43
Q

Presented by the formula (Ch2O)n, where n is the number of carbon atoms

A

Carbohydrates

44
Q

Are simple sugars, most common example is glucose

A

Monosaccharides
Mono- 1 sacchar- sweet

45
Q

Form when 2 monosacharrides undergo dehydration reaction

A

Disaccharides
Di- 2

46
Q

Includes fats, oils, waxes, phospholipids, and steroids

A

Lipids

47
Q

The building blocks of many hormones and is an important constituent of the plasma membrane

A

Lipids

48
Q

Are hydrophobic (water-fearing), insoluble in water and are nonpolar molecules.

A

Lipids

49
Q

Are one of the most abundant organic molecules in living systems and have the most diverse range of functions in all macromolecules

A

Protein

50
Q

Are the key macromolecules in the continuity of life.
Carries the genetic blueprint and the instructions for the functioning of the cell.

A

Nucleic Acid

51
Q

What are the 2 main types of nucleic acid

A

DNA- deoxyribonucleic acid
RNA- ribonucleic acid

52
Q

The genetic material found in all living organisms.
Ranging from single-celled bacteria to multicellular mammals

A

DNA

53
Q

Mostly involved in the protein synthesis.
Used by DNA to communicate with the rest of the cell.

A

RNA.

54
Q

two atoms of the same element share electrons, they are shared equally

A

Nonpolar covalent bond

55
Q

atoms of different elements share electrons, the shared electrons tend to be pulled closer to one element than the other (because of electronegativity)

A

polar covalent bond

56
Q

“Electrons shared evenly in the bond
-E-neg difference is zero or less than zero

A

Nonpolar bond

57
Q

Electrons unevenly shared
E-neg difference greater than zero but less than 2.0

A

Polar bond

58
Q

Molecules is nonpolar because it’s symmetrical

A

Nonpolar molecules

59
Q

-Not equal on all sides
•Polar bond between 2 atoms makes a polar molecule
-asymmetrical shape of molecule

A

Polar molecules/ dipoles

60
Q

Nonpolars are silimar
Polars are different

A

Bonds

61
Q

Nonpolar is symmetrical
Polar is asymmetrical

A

Molecules

62
Q

the electrons are not shared but transferred between atoms forming ions.

A

Ionic bond

63
Q

soluble in nonpolar liquids but not in water

A

Covalent compounds

64
Q
  • soluble in water but not in nonpolar liquid
A

Ionic compounds

65
Q

Happens when there is transferring or sharing of electrons

A

Chemical bonding

66
Q

Occurs between like atoms of a metal in the free state

A

Metallic bonding

67
Q

enable me-tals to conduct electricity

A

Mobile electrons

68
Q

-are called Salts or Crystals
-Always formed between metals and non-metals

A

Ionic bonding

69
Q

Pairs of e- are shared
between non-metal atoms

A

Covalent bonding

Gen chem (1 decks)

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