1: Atoms and Elements Flashcards

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1
Q

What is an atom?

A
  • Smallest particle of matter
  • Cannot be chemically divided
  • Atomos: indivisIble
  • Smallest component of an element
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2
Q

Explain Aristotle and Democritus’ views

A

A: atoms can be split forever (continuous theory), matter is divisible, 4 elements; water, fire, earth, wind
D: atoms cannot be split forever (discont.), matter is made of atoms, space between them, atoms can be different creating different objects/bodies

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3
Q

Define a theory, model, and law

A

Theory: “why?” beginning of an idea, set of principles explaining an aspect of reality
Model: manual made to see the inner workings of things too big or too small
Law: accepted statement explaining what’s happening based on data/observations

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4
Q

Explain Dalton’s theory

A

Atoms are empty, super tiny, can’t be divided, all atoms of the same element are identical, different atoms = diff. properties (mass, size), chemical reactions form new ones without creating, dividing, or destroying, only rearranging

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5
Q

What did Lavoisier theorize?

A

The law of conservation of matter: nothing is created, destroyed, only transformed. Total mass of reactants = total mass of product (first scientific theory on the nature of matter)

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6
Q

Explain Thomson’s theory

A

Cathode ray tube experiments leads to the discover of electrons (atoms emit light when electrified), proved that they’re neg. charged inside a pos. ball, follow a straight path, is divisible, plum pudding model

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7
Q

Explain Rutherford’s theory

A

Gold foil experiment, emitted alpha particles to the gold foil. most passed through but some bounced back or deflected, learned that they were mostly empty. but the matter was mostly concentrated in the middle: nucleus with pos. charge protons. Greater atom mass = bigger nucleus.

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8
Q

Explain the quantum theory

A

When an electron receives a quantum of energy, it jumps to a further orbital to release it and returns to its original shell. This distance creates a light wave of colour.

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9
Q

What is the periodic table?

A

It is a way to classify elements according to certain patterns in their properties, both chemical and physical

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10
Q

Describe Metals and its location on the table

A

To the left of the staircase

  • Good conductors (elec., heat)
  • Ductile and malleable
  • Shiny
  • Solid at room temp (except mercury)
  • Many react with acids, release hydrogen
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11
Q

Describe NonMetals and its location

A

To the right of the staircase

  • Poor conductors
  • Brittle, dull
  • Mostly gasses at room temp.
  • No reactions to acid
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12
Q

What is an alloy?

A

A mixture of metals/non metals, combining qualities from all the elements they’re composed of

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13
Q

Describe metalloids and their location

A

On either side of the staircase, have properties of both other categories, ex: pyrex in cookware

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14
Q

Why is hydrogen #1 on the periodic table?

A

Though it is a nonmetal, it is located in column one due to its properties and atomic structure (1 v. e.)

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15
Q

Why are elements in groups (columns)?

A

Elements have the same chemical properties because they have the same # of v. e.

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16
Q

What signifies a stable atom?

A

When the valence shell is full by gaining, losing, or sharing electrons during a chemical reaction (whichever is easiest) ie: 2 v.e. will lose 2, 6 v.e. will gain 2. This is how bonds form to create molecules.

17
Q

What signifies an atom’s chemical reactivity?

A

How fast it can gain/lose v.e. (the faster, the higher the reactivity) 1v.e./7v.e. are more reactive cause they are closer to reaching a full shell

18
Q

What are the octet and duet rules?

A
Octet: needs a full valence shell of 8 v.e.
Duet rule (H, Li, He, B, Be): full valence shell of 2 v.e.
19
Q

Describe alkali metals

A
  • G1A, except H
  • Soft, light
  • Low melting point
  • Excellent conductors
  • Highly reactive (stored in oil to avoid contact w air moisture)
  • Found in halogen compounds, forming salts,
20
Q

Describe alkaline earth metals

A
  • G2A
  • Harder, malleable, grey
  • High melting point
  • Excellent conductors
  • Less violent reactions (burn easily but can be exposed to air)
  • Found in rock compounds
  • Halogen compounds forming salts
21
Q

Halogens

A
  • G7
  • Coloured
  • React easily to alkali metals, forming compounds (salts)
  • React w hydrogen to form acids
  • Toxic, corrosive, bactericidal
22
Q

Noble gases

A
  • G8
  • Colourless
  • Emit colour when electrified (quantum theory)
  • Stable, full shell (low reactivity)
  • Found in elemental state in nature
23
Q

What is an isotope?

A

Forms of an element with different numbers of neutrons, same chemical properties but different physical properties

24
Q

What is the atomic radius trend?

A

More protons = more attraction between e. and nucleus. Higher attraction = smaller nucleus since it’s pulled more tightly tgt. Within a period, the atomic radius decreases. Going down a group it increases because the number of shells gets bigger.

25
Q

What is the ionization energy trend?

A

Energy required to remove the outermost electron from its atoms, thus creating an ion: atom with a charge else than zero. Higher ion energy = more energy required to remove an electron since it is more attracted to the nucleus. IE increase as AR decreases

26
Q

What is the electronegativity trend?

A

Attraction to another atom’s electrons. How likely it is to gain electrons. Higher value = more likely to gain. The less shells, the closer the electrons, higher attraction. EN is higher at the right of the periodic table, since they almost have a full shell.

27
Q

What is the chemical reactivity trend?

A

How likely/vigorously an atom will react with other substances based on the number of v.e.. The closer they are to obtaining a full shell, the more reactive.

28
Q

What is lewis notation?

A

Symbol + number of v.e. surrounding it’s “four walls” with dots