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Atoms and Elements - Atomic Theory Flashcards

(44 cards)

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1
Q

What is an atom?

A

-the smallest part of an element that can exist
-‘atom’ comes from the Ancient Greek adjective ‘Atomos,’ which means indivisible or not to be cut

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2
Q

What is an element?

A

-a pure form of matter that cannot be broken down into simpler substances
-only one type of atom
-there are 118 elements

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3
Q

What important information does the Periodic Table tell us about the atoms of elements?

A

-how many protons + electrons + neutrons it has

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4
Q

How has the concept of an atom changed over time?

A

-the concept of an atom has changed over time as more and more research has been done and theories have evolved

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5
Q

Democritus

A

-400 BC
-shaded sphere
-analogy is Lego bricks

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6
Q

Aristotle

A

-300 BC
-fire, dry, earth, cold, water, wet, air, hot - model
-RIP - headstone - analogy

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7
Q

Dalton

A

-1803
-shaded sphere with shadow
-8 ball - analogy

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8
Q

Thomson

A

-1897
-spherical cloud of positive charge with circles (electrons)
-chocolate chip cookie - analogy

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9
Q

Rutherford

A

-1908
-the nucleus, electrons on orbits around it
-cherry with a pit - analogy

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10
Q

Bohr

A

-1913
-Bohr Model (rings/energy levels/shells with electrons (2,8,8,8)
-Solar System - analogy

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11
Q

Schrodinger, Heisenberg, Einstein, and other scientists

A

-modern (now)
-20th century
-modern cloud theory
-shaded circle (electron cloud) with nucleus in the middle
-cotton ball - analogy

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12
Q

What are subatomic particles?

A

-protons (positive charge), neutrons (neutral charge), and electrons (negative charge)

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13
Q

Proton

A

-positive charge (+)
-p+
-1 amu (atomic mass unit) - mass

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14
Q

Neutron

A

-neutral charge (0)
-n*
-1 amu

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15
Q

Electron

A

-negative charge (-)
-e-
-0 amu

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16
Q

amu=

A

-atomic mass unit
-a tiny unit of mass used to measure the mass of subatomic particles

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17
Q

Where are the subatomic particles?

A

-protons and neutrons are packed into the extremely dense nucleus at the center if the atom
-electron - cloud
-‘massless’ electrons circle the nucleus billions of times per second

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18
Q

What are isotopes?

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A

-atoms of the same element that have different numbers of neutrons

19
Q

What information do Periodic Table squares tell us about elements?

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A

-state at room temperature - solid, liquid, gas
-atomic number - identity of element, how many protons atoms of the element have
-atomic mass - average mass of isotopes of element
-mass number - rounded atomic mass
-element name
-chemical symbol - one or two-letter symbol that represents the element (first letter always capitalized)

20
Q

What is a group?

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A

-each column down the table is called a group
-the elements in a group have a lot of properties in common
-there are 18 groups

21
Q

What is a period?

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A

-each row across the table is called a period
-there are 7 periods

22
Q

How do scientists organize the elements on a chart?

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A

-scientists needed a good chart to help them organize what they knew about the chemical elements
-in 1869, a Russian chemist named Dmitri arranged all 60 of the known elements into a table
-Mendeleev organized them by atomic masses, and he left blanks in the spaces for elements that were not yet discovered

23
Q

What is the Periodic Table?

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A

-a chart that helps organize what we know about chemical elements

24
Q

Chemical Symbol

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A

-a one or two letter symbol that represents the element

25
What does periodic mean?
-means to be "repeated in a pattern"
26
What are metals?
-share certain properties -solid at room temp. -silver-gray except gold and copper -certain shiny look called metallic luster -good conductors of heat and electricity -malleable - you can press them into new shapes without them breaking -ductile - you can pull them to create wires
27
What are nonmetals?
-some are solids at room temp. -others are liquids -many are gases many colors including yellows, dark red, white, and also colorless -do not have metallic luster and tend to look dull -poor conductors of heat and electricity -not malleable or ductile but instead break apart when hammered or pulled
28
What are metalloids?
-solid at room temp. -have metallic luster and generally look like metals -brittle and easily shattered -can conduct electricity, but not as well as metals
29
What are the types of elements on the Periodic Table?
-metals - left side of staircase - more than nonmetals -nonmetals - right side of the staircase -metalloids - along the staircase -hydrogen is a nonmetal but it can act like a metal and it's the lightest element so it's located at very top left
30
What are the element families of the Periodic Table?
-Alkali Metals -Alkaline Earth Metals -Transition Metals -Poor Metals -Metalloids -Halogens -Noble Gases -Lanthanides -Actinides -Other Nonmetals
31
How can we model atomic structure to help predict how atoms behave?
-the current atomic model is known as the 'electron cloud model,' which includes a very tiny nucleus surrounded by electrons moving close to the speed of light -this model is difficult to study -the 'Bohr-Rutherford' or 'Bohr Diagram' model of the atom is like taking a picture of an atom in a given moment -it's a way of representing the most likely locations of electrons in the 'cloud'
32
Model
-a visual and simpler way to represent a complex, large, or small concept
32
Why are atomic models used?
-atoms are so small that in order to study them, we need to create models
33
What are the parts of a Bohr model?
-nucleus - the nucleus can be represented by the number of protons and neutrons -electrons - the electrons are shown very big and bold so that they're easy to count -electron shells - also known as 'levels' electrons orbit the nucleus on specific shells
34
How does an electron's location correspond to its energy?
-imagine going up a ladder. As you go up each ring, you gain more and more potential energy to fall -this is similar to the way in which electrons have more energy as they orbit farther from the nucleus -the shells of an atom are named K, L, M, and N, going from the closest to farthest from the nucleus
35
How do electrons fill the shells in atoms with atomic numbers 1 through 20?
-electrons fill the K shell (level 1) first. The K shell is full when it has just TWO electrons -remaining electrons fill the L shell (level 2) next. The L shell is full when it has EIGHT electrons -any remaining electrons fill the M shell (level 3) next. For the first 20 elements, the M shell is full when it has EIGHT electrons -if there are still remaining electrons, they fill the N shell (level 4). The N shell is full when it has EIGHT electrons
36
How is a Bohr diagram drawn?
-write the element's symbol with the mass number at the top left and the atomic number at the bottom left (this is called shorthand) -calculate the number of neutrons in the atom -write the number of neutrons and protons (p+ and n0) as the nucleus -draw the K shell and fill it with the first 2 electrons -continue drawing each shell and filling with electrons until you have accounted for all of the atom's electrons
37
The property that means a certain shine that a metal has
-metallic luster
38
The elements are located in certain groups and families based on their
-properties
39
The property that means the substance can be easily flattened or shaped without breaking
-malleable
40
If heat and electricity run easily through it, then it's a good
-conductor
41
On either side of this feature of the Periodic Table are the metalloids
-staircase
42
The elements of the first Periodic Table were arranged by
-atomic mass
43
How do you calculate how many neutrons are in the atom?
mass number - atomic number = # of neutrons

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