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CHEMISTRY 60 > CHAPTER THREE: ATOMS AND ELEMENTS > Flashcards

CHAPTER THREE: ATOMS AND ELEMENTS Flashcards

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1
Q

What are the capitalization rules for chemical symbols on the periodic table?

A

Chemical symbols are 1 or 2-letter abbreviations for the names of the elements. Only the first letter of an element’s symbol is capitalized. If the symbol has a second letter it is lowercase so that we know when a different element is indicated.

If two letters are capitalized, they represent the symbols of two different elements!

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2
Q

Each horizontal row on the Periodic Table is called a _________ and there are a total of _____.

A

PERIOD

7

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3
Q

Each vertical column on the Periodic Table contains a __________ of elements that have similar ___________.

A

GROUP

Properties

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4
Q

Where are the REPRESENTATIVE ELEMENTS located on the Periodic Table and how are they numbered?

A

The elements in the first 2 columns on the left and the last 6 columns on the right of the periodic table are called the REPRESENTATIVE ELEMENTS (given group numbers 1A-8A).

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5
Q

Where are the TRANSITION ELEMENTS located on the Periodic Table and how are they designated?

A

In the center of the Periodic Table is a block of elements known as the TRANSITION ELEMENTS (designated with the letter “B”)

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6
Q

The ___________ and ___________ that are part of Periods 6 and 7 are placed at the bottom of the Periodic Table to allow it to fit on a page.

A

lanthanides and actinides

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7
Q

What is the name of the group 1A elements?

A

It is a family of elements called the ALKALI METALS (soft, shiny, good conductors of heat and electricity).

Hydrogen is at the top of Group 1A but is not an alkali metal.

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8
Q

What is the name of the group 2A elements?

A

These are called the ALKALINE EARTH METALS. Shiny metals, but not as reactive.

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9
Q

What is the name of the elements in group 7A?

A

The HALOGENS are highly reactive and form compounds with most of the elements.

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10
Q

What is the name of the elements in group 8A?

A

the NOBLE GASES are quite unreceptive and are seldom found in combination with other elements.

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11
Q

Another feature of the periodic table is the heavy zigzag line that separates the elements into the _______ (on the left of the line except for hydrogen) and the _______ (on the right of the line).

A

The METALS and the NONMETALS

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12
Q

What are the general characteristics of the METALS?

A

Most are:

  • shiny solids
  • ductile (can be shaped into wires) or malleable (hammered into a flat sheet).

They are good conductors of heat and electricity and usually melt at higher temperatures than nonmetals.

All are solids at room temperature except for mercy (Hg), which is a liquid.

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13
Q

What are the general characteristics of the NONMETALS?

A

They are not especially shiny, ductile or malleable, and they are often conductors of heat and electricity. They typically have low melting points and low densities.

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14
Q

What are the METALLOIDS?

A

Except for aluminum, the elements located along the heavy line are METALLOIDS.

These are elements that exhibit some properties that are typical of the metals and other properties that are characteristic of the nonmetals. They are better conductors of heat and electricity than the nonmetals, but not as good as the metals.

They are semi-conductors because they can be modified to function as conductors or insulators.

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15
Q

All the elements listed on the Periodic Table are made up of ___________.

A

ATOMS

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16
Q

What is an ATOM?

A

The smallest particle of an element that retrains the characteristics of that element.

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17
Q

What is the significance of Dalton’s Atomic Theory?

A

It formed the basis of current atomic theory. Dalton lived 1766-1844

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18
Q

What are SUBATOMIC PARTICLES? Name three of them.

A

Atoms are composed of even smaller bits of matter called SUBATOMIC PARTICLES- three of which are the PROTON, NEUTRON and ELECTRON.

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19
Q

__________ are subatomic particles that are negatively charged.

A

ELECTRONS

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20
Q

________ are subatomic particles that are positively charged.

A

PROTONS

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21
Q

The center of the atom is called the ______.

A

NUCLEUS

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22
Q

The nucleus of the atom contains a subatomic particle that is neutral that is called a ____________.

A

NEUTRON

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23
Q

Because the masses of subatomic particles are so small, chemists use a very small unit of mass called an ________ _______ ______ (abbreviation= __________).

How is this unit defined?

A

ATOMIC MASS UNIT ( amu)

An amu is defined as one-twelfth of the mass of a carbon atom which has a nucleus containing six protons and six neutrons.

On the amu scale, the proton and newborn each have a mass of about 1 amu.

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24
Q

All the atoms of the same element always have the same number of __________, which is a feature that distinguishes atoms of one element from atoms of all the other elements.

A

PROTONS

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25
Q

What is an ATOMIC NUMBER?

A

An atomic number, which is equal to the number of protons in the nucleus of an atom, is used to identify and define each element.

Atomic number = number of protons in an atom

The atomic number is the whole number that appears above the symbol of each element.

Ex: A hydrogen atom, with atomic number 1, has 1 proton. An atom of carbon, with atomic number 6, has 6 protons.

26
Q

An atom is electrically ________.

In every atom, the atomic number also gives the number of ___________.

A

NEUTRAL. The number of protons in an atom is equal to the number of electrons. This electrical balance gives an atom an overall charge of zero.

Thus, in every atom, the atomic number also gives the number of ELECTRONS.

27
Q

The protons and neutrons determine the mass of the nucleus. For any atom, the ____ number is the sum of the number of protons and neutrons in the nucleus of a single atom.

This is a __________ number and is always a ________ number.

Does the mass number appear on the Periodic Table?

A

the MASS number

a COUNTING number and is always a WHOLE number.

It does NOT appear on the Periodic Table because it represents the particles in the nucleus of a single atom.

Mass number=
number of protons + number of neutrons

28
Q

Atoms of any one element are not completely identical because they can have different numbers of _________.

A

NEUTRONS

29
Q

What are ISOTOPES?

A

They are atoms of the same element that have the same number of protons but different numbers of neutrons.

30
Q

How do we distinguish between the different isotopes of the same element?

A

Write an ATOMIC SYMBOL that indicates the mass number of each isotope in the upper left corner and the atomic number of the element in the lower left corner.

Ex: the atomic symbol for an isotope of magnesium (note that the numbers should be written closer together than I can do it here on this card)

24
Mg
12

31
Q

How do we refer to an ISOTOPE?

A

An isotope may be referred to by it’s NAME or SYMBOL followed by the mass number.

Ex: Magnesium
* magnesium-24 OR Mg-24

32
Q

In a large sample of naturally occurring isotopes of a particular element, each type of isotope can be present in _________ percentages.

A

VARYING (low or high percentage)

For example: the Mg-24 isotope makes up almost 80% of the total sample, whereas Mg-25 and Mg-26 each make up only about 10% of the total number of magnesium atoms.

33
Q

Because each isotope has a different mass, chemists have calculated an ______ _____ for an “average atom”, which is a weighted average of the masses of all the naturally occurring isotopes of that element.

On the Periodic Table, this is the number including decimal places that is given below the symbol of each element.

A

ATOMIC MASS

NOTE: most elements consist of two or more isotopes, which is one reason that the atomic masses on the Periodic Table are seldom whole numbers

34
Q

CALCULATING ATOMIC MASS:

To calculate the atomic mass of an element, the percentage abundance of each isotope and its mass must be determined _______.

A

…must be determined EXPERIMENTALLY.

See page 104 in Melbardis text for example

35
Q

What is ELECTROMAGNETIC RADIATION?

What is the WAVELENGTH?

All forms of electromagnetic radiation travel in space at the speed of __________ but differ in ________ and ____________.

A

Light and other electromagnetic radiation consist of energy particles that move as waves of energy.

The distance between the peaks is called the WAVELENGTH.

The speed of LIGHT (3.0 x 10^8 m/s); differ in ENERGY and WAVELENGTH. (high-energy radiation has short wavelengths compared to low-energy radiation, which has longer wavelengths)

36
Q

What is the ELECTROMAGNETIC SPECTRUM?

What is the ATOMIC SPECTRUM?

A

The ELECTROMAGNETIC SPECTRUM shows the arrangement of different types of electromagnetic radiation in order of increasing energy.

When light from an element that is heated passed through a prism, it separates into distinct lines of color called an ATOMIC SPECTRUM. Each element has its own unique atomic spectrum.

37
Q

In an atom, each ELECTRON has a specific energy known as its ________ _______.
(All the electrons with the same energy are group in the same one).

Describe the bookcase analogy for this.

What are some differences from the analogy?

A

ENERGY LEVEL

Analogy: think of energy levels as similar to the shelves in a bookcase. The lowest shelf is the lowest energy level (takes less energy to fill the bottom shelf first). We could never get any book to stay in the space between shelves- its the same with the energy of an electron- it must be at specific energy levels, and not between.

Unlike the analogy:

  • there is a large difference between the energy of the first and second levels, but then the higher energy levels are closer together.
  • the lower electron energy levels hold fewer electrons than the higher energy levels.
38
Q

ENERGY LEVELS are assigned numbers (n) beginning with __________ up to _______

A

n = 1, n= 2, up to n = 7

39
Q

Which are closer to the nucleus?

  • electrons in the lower energy levels
  • electrons in the higher energy levels
A

Electrons in the lower energy levels

40
Q

How does an electron change from one energy level to a higher level?

How does an electron change from one energy level to a lower level?

If the energy emitted is in the visible range, we see _______________.

A

It can only change to a higher level if it absorbs the energy equal to the difference between two levels.

When it changes to a lower energy level, it emits energy equal to the difference between the two levels.

…we see one of the colors of visible light (Ex: the yellow color of sodium streetlights; the red color of neon lights)

41
Q

What is meant by the ELECTRON ARRANGEMENT of an atom?

A

The ELECTRON ARRANGEMENT of an atom gives the number of electrons in each energy level.

42
Q

We can write the ELECTRON ARRANGEMENTS for the first 20 elements by _____________________.

A

…by placing electrons in energy levels beginning with the lowest.

43
Q

Is there a limit to the number of electrons allowed in each energy level?

A

YES.

Only a few electrons can occupy the lower energy levels, while more electrons can be accommodated in higher energy levels.

44
Q

How many electrons can be held in each energy level?

  • energy level 1
  • energy level 2
  • energy level 3
  • energy level 4
A
  • energy level 1 can hold 2 electrons
  • energy level 2 can hold 8 electrons (2+6)
  • energy level 3 can hold 18 electrons
    (2+6+10)
  • energy level 4 can hold 32 electrons
    (2+6+10+14)
45
Q

What are PERIODIC PROPERTIES?

What are 3 periodic properties?

Each of these _______ or ________ across a PERIOD, and then the trend is _____ _______ in each successive period.

A

The electron arrangements of atoms are an important factor in the PHYSICAL and CHEMICAL properties of elements.

VALENCE ELECTRONS in atoms, ATOMIC SIZE and IONIZATION ENERGY.

Each of these INCREASES or DECREASES across a period, and then the trend is REPEATED AGAIN in each successive period.

46
Q

The CHEMICAL PROPERTIES of representative elements in Groups 1A (1) to 8A (18) are mostly due to the _____ _____, which are the _________________.

A

VALENCE ELECTRONS, which are the electrons in the outermost energy level.

47
Q

The ______ ________ gives the number of VALENCE ELECTRONS for each group of representative elements.

How many valence electrons do the elements in these groups have?

  • Group 1A (1)
  • Group 2A (2)
  • Group 7A (17)
A

GROUP NUMBER

  • Group 1A (1)= one valence electron
  • Group 2A (2)= two valence electrons
  • Group 7A (17)= seven valence electrons
48
Q

What is an ELECTRON-DOT SYMBOL?

How are they arranged?

A

Represents the valence electrons as dots that are placed on the sides, top or bottom of the symbol for the element.

One to four valence electrons are arranged as single dots. When an atom has 5-8 valence electrons, one or more electrons are paired.

See examples on page 113 Melbardis text

49
Q

The size of an atom is determined by its _______ _______, which is the ______.

For each group of representative elements, the atomic size _________ from the top to the bottom because ____________.

Example- comparing three elements from Group 1A to determine the relative size:

  • Li
  • Na
  • K
A

ATOMIC RADIUS- the distance of the outermost electrons from the nucleus.

INCREASES…. because the outermost electrons in each energy level are farther from the nucleus.

Example:

  • Li has a valence electron in energy level 2
  • Na has a valence electron in energy level 3
  • K has a valence electron in energy level 4
  • this means that a K atom is larger than a Na atom, and a Na atom is larger than a Li atom.
50
Q

For the elements in a period, an increase in the number of protons in the nucleus _________ the attraction for the outermost electrons.

As a result, the outer electrons are ___________ the nucleus, which means that the size of representative elements ______ going from left to right across a period.

A

INCREASES

PULLED CLOSER TO the nucleus, which means that the size of representative elements DECREASES going from left to right across a period.

51
Q

In an atom, negatively charged electrons are attracted to the positive charge of the protons in the nucleus. Thus, a quantity of energy known as the _______ _______ is required to _______ one of the outermost electrons.

When this happens to a neutral atom, a positive particle called a __________ with a _________ charge is formed.

A

A quantity of energy known as the IONIZATION ENERGY is required to REMOVE one of the outermost electrons.

CATION; 1+ charge

52
Q

The IONIZATION ENERGY _________ going down a group. Explain this….

A

DECREASES

Less energy is needed to remove an electron because because nuclear attraction decreases when electrons are farther from the nucleus.

53
Q

The IONIZATION ENERGY ______ going across a period from left to right.

Explain this….

A

INCREASES

As the positive charge of the nucleus increases, more energy is needed to remove an electron.

54
Q

In Period 1, the valence electrons are close to the nucleus and strongly held. H and He have _____ IONIZATION ENERGIES because ____________________

The ionization energy for He is the _______ of any element because He has a full, stable, energy level which is disrupted by removing an electron.

The _______ ionization energies of the noble gases indicate that their electron arrangements are especially _________.

In general, the ionization energy is _____ for the metals and _____ for the nonmetals.

A

HIGH ionization energies…. because a large amount of energy is required to remove an electron.

HIGHEST

HIGH; stable

LOW; HIGH

55
Q

An element that has METALLIC CHARACTER is an element that ______________.

This is more prevalent in the elements (______) on the left side of the Periodic Table and _____ going from the left side to the right side of the periodic table.

The elements (_________) on the right side of the Periodic Table __________ easily lose electrons

A

Loses valence electrons EASILY.

METALS; DECREASES

NONMETALS: do not easily lose electrons (can’t read the scanned page 116 for the rest of this… can you get a new scan?)

56
Q

Developmental History of the Atom:

* Thompson

A
  • Thompson- discovery of the electron (1897), first evidence for isotopes of stable element (1913), invented mass spectrometer, plum pudding model
57
Q

Developmental History of the Atom:

* Rutherford

A
  • Rutherford- (1909) planetary model of the atom (all protons in the nucleus and electrons orbiting)
58
Q

Developmental History of the Atom:

* Bohr

A
  • Bohr (1913)-a picture of atomic structure, size of the orbit is only important info (n quantum)
59
Q

Developmental History of the Atom:

* Schrodinger

A
  • Schrodinger (1926)- electron is a wave
60
Q

1 amu= ____ grams

A

1.661 x 10^-24 grams

CHEMISTRY 60 (18 decks)

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