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atomic structure Flashcards

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1
Q

Who were the first people to proprose that matter was made up of particles of elemental substances?

A

The greeks

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2
Q

What became of the Greek views of matter?

A

it faded

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3
Q

What were Democritus (460-370) ideas about matter?

A
  1. smallest paticles of matter are called atoms
  2. different type of atoms for every type of matter
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4
Q

Democritus ideas about matter were not useful in a scientific sense. why?

A
  1. no experimental evidence to support it
  2. did not explain the chemical behavior of atom
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5
Q

What did Robert Boyle do in the 1600s?

A

showed that gold and silver were elements and are not made up of fire, water, wind and earth

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6
Q

What was Dalton’s model of atom? What was it’s purpose?

A
  1. cannon ball
  2. proposed that atoms were tiny hard sphere
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7
Q

Which sub-atomic particle is the first to be discovered in the atom?

A

The electron in 1871

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8
Q

Who discovered the electrons?

A

J.J Thompson

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9
Q

Who made the plum pudding?

A

J.J Thompson

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10
Q

Which scientist 1st discovered the nucleus?

A

Ernest Rutherford in 1911

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11
Q

HOw did he discover the nucleus?

A

By finding alpha particles at gold foil

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12
Q

What did Rutherford observed?

A
  1. most alpha particles went straight through the gold foil
  2. only a few alpha particles wee deflected when they came close center of the atom
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13
Q

Why most alpha paticles passed straight through the gold foil?

A

b/c atoms is mainly made up of empty spaces

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14
Q

Why were a few alpha particles deflected?

A

b/c of repulsion between the alpha particles and the central core of atom

pos + pos = repulsion

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15
Q

What is the atom mostly made up of?

A

empty spaces

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16
Q

What are the characteristics of the nucleus?

size, density, location, charge

A
  1. much smaller than atom
  2. very dense, contains most of the atoms mass
  3. center of the atom, central core of the atom
  4. positive charge
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17
Q

What did Bohr proposed about atoms?

A

The atom has a very small, positively charged nucleus. Surrounded by electons orbiting the nucleus in energy levels

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18
Q

What was Bohr’s model of atom called?

A

The Planetary MOdel

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19
Q

WHy was Bohr’s model of the atom not accepted?

A

b/c experimental evidence did not support it

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20
Q

Wave Mechanical Model ( current model)

( 5 bullet points)

A
  1. matter consists of mass of partiles
  2. energy consists of waves
  3. evidence showed that the electron has both mass and wave like properties( dual nature)
  4. this dual nature of the electron has been incorporated in the most of the most curren model of atom called wave mechanical model
  5. in the wave mechanical model the electrons are located in orbitals
21
Q

What are oribitals?

A

Orbitals are regions in which the electrons are most likely or probably to found. In the orbitals the electrons move with distinct energy

22
Q

Describe an atom.

( 2 bullet points)

A
  1. atom is the smallest particle of an element that etains the chemical properties of that element
  2. contgains a small dense, positively charged nucleus srrrounded by a large space occupied by electrons
23
Q

What particles are found in the nucleus?

A
  1. protons and nuetrons
  2. the particles found in the nucleus are collectively called nucleons
  3. # of nucleons = # of protons + # of neutrons
24
Q

What is the overall charge of an atom?

A

over charge - all atoms is electrically neutral or zero

25
Q

what is the formula to the overall charge of the nucleus?

A

nucleus charge = # of protons in nucleus

26
Q

WHat is meant by the term “atomic number?”

A

this is the number or protons in the nucleus of an atom

atom # = # of protoms

27
Q

why don’t two elements have the same atomic number?

A

because each element has a unique number of protons in its nucleus, no two elements have the same atomic #

28
Q

What is meant by the term “ mass number”

A

sum of protons and neutons in the nucleus of an atom

mass number = # of protons + # of neutrons

29
Q

how do we find the number of neutrons?

A

neutrons = mass # - atomic #

30
Q

Where outside the nucleus are the electrons to be found?

A
  1. electrons ae found outside the nucleus in principle energy levels or shells
  2. each principal energy level can only hold a certain amount of electrons
31
Q

Principal energy level (n)

n = 1 energy level

n=2 energy level

n=3 energy level

n= 4 energy level

A
  1. 2
  2. 8
  3. 18
  4. 32
32
Q

which electron enery level has the lowest energy

A

1st energy level

33
Q

what is meant by tht eterm electon configuration?

A

Electon configuration shows the distribution of electons in an atom

34
Q

What are valence electrons?

A

Valence electrons are electrons in the outermost principal energy or shell

# of valence electrons = # of electrons in the outemost shell

35
Q

What is the Lewis Dot Diagram ?

A

consists of a chemical symbole surounded by one to eight dots representing valence electrons

36
Q

What are isotopes?

A

Isotopes are atoms of the same element that have the same number of protons and electrons but different number of neutrons

OR

Isotops are atoms of the same element of having the same atomic number different mass number

37
Q

What is atomic mass?

A
  1. the atomic mass of an element is the average mass of all naturally occuring isotops of that element
  2. the atomic mass of an element is usually closest to the isotope with the highest natural abundance
38
Q

What are electrons said to be in ground state?

A

when they occupy the lowest available energy levels

39
Q

What happens when energy ( heat, light or electic) is applied to electons in the gound state?

A

The electrons in the ground state absorbs the energy and move up to higher energy level

40
Q

What are these higher energy level called?

A

Excited states

41
Q

Describe the electrons in excited states

A

electrons in the excited states have high energy and are very unstable

42
Q

What will eventually happen to the electrons in the excited state?

A

They quickly return to the ground state by releasing energy to the form of light

43
Q

WHat are the lines called shown through a spectroscope?

A

bright line spectrom or emission lines

44
Q

Why are spectral lines known as fingerprints of elements?

A

Each element has its own unique bright line spectrum

45
Q

What is an ion?

A

an ion is an electrically charged particle

46
Q

What charge can an ion have?

A

positive and negative

47
Q

Describe a positive ion

(3 bulletpoints)

A
  1. A positive ion will have more psitively charged protons than negatively charge electrons
  2. positive ions called cations
  3. positive ions are formed when an atom loses lectrons there ions how formed will have more portons than electrons
48
Q

Describe negative ions

(3 bulletpoints)

A
  1. a negative ion will have more negatively charge electrons than positively charge protons
  2. negative ions called anions
  3. negative ions are formed when an atom gains electrons therefore the ion now formed will have more electrons than protons

chemistry (14 decks)

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