Chemistry Chap 2:the Structure Of The Atom And The Periodic Table

Front 1

Atom

Back 1

The basic structural unit of an element and the smallest particle of an element that retains the chemical properties of that element.

Hint 1

39

Front 2

What three primary particles are atoms composed of?

Back 2

The protons, neutrons, and electrons.

Hint 2

39

Front 3

Atoms are composed of how many distinct regions?

Back 3

two: the nucleus and the region outside of the nucleus

Hint 3

39

Front 4

Nucleus, protons, and neutrons

Back 4

The nucleus is a small, dense, positively charged region in the center of the atom. The nucleus is composed of positively charged protons and uncharged neutrons.

Hint 4

39

Front 5

Electrons

Back 5

Surrounds the nucleus in a different region of negative charge electrons.

Hint 5

39

Front 6

atomic number

Back 6

Number of protons in the atom.

Hint 6

39

Front 7

mass number

Back 7

The sum of the number of protons and neutrons.

Hint 7

39

Front 8

The number of electrons is equal to the amount of (in a neutral atom)=

Back 8

protons.

Hint 8

40

Front 9

Isotopes

Back 9

Atoms of the sames element having different masses because they contain different numbers of neutrons. Isotopes have different mass numbers.

Hint 9

40

Front 10

Ions

Back 10

Electrically charged particles that result from a gain of one or more electrons by the parent atom (forming negative ions, or anions) or a loss of one or more electrons from the parent atom (forming positive ions, or cations).

Hint 10

40

Front 11

Periodic law

Back 11

If the elements are arranged according to their atomic numbers, there is a regular variation of their physical & chemcial properties.

Front 12

Mendeleev orginal periodic table as arrange...

Back 12

in order of increasing atomic mass with elements with similar properties grouped together in what was the first periodic table. Same way we do it today!!!

Hint 12

53

Front 13

Modern periodic law

Back 13

The physical and chemical properties of the elements are periodic functions of their atomic numbers.

Front 14

In the periodic table the horizontal rows are called __________.

Back 14

periods.

Hint 14

55

Front 15

metals vs nonmetals

Back 15

A metal is a subtance that tend to lose electrons during chemical change, forming positive ions. A nonmetal, on the other hand, is a substance whose atom may gain electrons forming negative ions.
-metals are shinny, are malleable; are ductile, are good conductors of heat and electricity; and most are solids at room temp.
-nonmetals are NOT shiny, are NOT malleable; are NOT good conductors of heat and electricity; and several are gases at room temp.

Hint 15

55

Front 16

electron configuration

Back 16

The arrangement of electrons around a nucleus of an atom, ion, or a collection of nuclei of a molecule.

Hint 16

g-4

Front 17

Valence electrons

Back 17

The outermost electrons in an atom, which are involved, or have the potential to become involed in the bonding process.

Hint 17

58

Front 18

In the periodic table the vertical rows are called

Back 18

group or familes.

Front 19

Sub level

Back 19

Set of equal-energy orbitals within a particular energy level.

Hint 19

61

Front 20

Octet rule
metals vs nonmetals with octet rule

Back 20

-Element usually react in such a way as to attain the electron configuration of the noble gas closest to them in the periodic table.
-Metal, having a small number of valence electrons, tend to lose their valence electrons forming cations.
-Nonmetals, having a large number of valence electrons, tend to react with metals by gaining enough electrons to reach the noble gas electron configuration or 8 valence electrons, forming anions.
-Sometimes nonmetals will share valence electrons with other nonmetals to attain the noble gas electron configuration.

Hint 20

65

Front 21

The nucleus is __________ smaller than the atom as a whole.

Back 21

10,000 times

Front 22

The representation of an element using symbol is usually in order of:

Back 22

Symbol in the midder. To the left side is mass number on top, and atomic number on the bottom. To the right is the charge on the top.

Front 23

Dalton's Atomic Theory

Back 23

1)All matter is made up of tiny particles called atoms.
2)An atom can not change, divided, destroy or convert to any other type of atom.
3)All atoms of an element are identical in every way.
4)Atoms of different elements have different properties.
5)Atoms of different elements can combine in simple whole-number ratios, to form compounds.
6)A chemical change occurs when atoms joined, separated, or rearranged.

Front 24

Which of Dalton's Theory is still consisder true?

Back 24

1,4,5,6 are still consider true.

Front 25

What eveidence is there of subatomic particles?

Back 25

J.J. Thompson:cathode ray tubes; electrons, and Rutherford:gold foil experiment; nucleus.

Front 26

wavelength

Back 26

The distance frome the beginning of a wave to the beginning of another wave or the distance from crest to crest. the upside down v symbol

Front 27

Radiowave: Frequecy

Back 27

Is the number of waves passing a point in a given amount of time. the v symbol

Front 28

speed of light

Back 28

Is the product of wavelength and the fequency, is a constant; c=3.00 x 10 to the 8th m/s

Front 29

-the energy, E, of the speed of light is found by...

Back 29

multiplying the frequency by Planck's constant, h
h=6.63x10 to the -34 Js
E=(h)(v)

Front 30

Electromagnetic Spectrum high energy to low energy list:

Back 30

Gamma rays, X-ray, ultraviolet light, visible light, infrared light, microwaves, radio waves

Front 31

metalloids(mět'l-oid')

Back 31

Elements that border the zigzag line, they have properties intermediate between metals and nonmetals, except aluminum which is classified as a metal.

Front 32

What is the only nonmetal element to the left of the zigzag line on the periodic table?

Back 32

H-Hydrogen

Front 33

Ion size

Back 33

-Decrease in size from Left to right.
-Increase in size from top to bottom.
-Some exceptions exist.

Front 34

ionization energy

Back 34

The energy required to remove an electron from an isolated atom.
-Reading down a group, the ionization energy decreases, because of the atom's size increases. The outermost electron is progressively farther from the nuclear charge, hence easier to remove.
-Reading across a period, the ionization energy increase, note that atomic size decreases, because the outer most electrons are close to the nucleus, thus harder to remove.

Front 35

electron affinity

Back 35

The energy released when a single electron is added to an isolated atom.
-Electrons affinities generally decrease down a group.
=Electrons affinities generally increase across a period.

Front 36

Filling order for electrons

Back 36

1s
2s 2p
3s 3p 3d
4s 4 p 4d 4f

Amount of orbitals
s-1,p-3,d-5,f-7

Front 37

Where are Alkali metals located?

Back 37

Group IA

Front 38

Where are Alkaline earth metals located?

Back 38

Group IIA

Front 39

Where are Noble gases located?

Back 39

Group VIIIA

Front 40

Where are Halogens located?

Back 40

Group VIIA

Front 41

Groups A

Back 41

Representative elements

Front 42

Groups B

Back 42

Transition elements

Front 43

Period 6 and 7

Back 43

Inner Transition elements

Front 44

What is the shape of the s orbital?

Back 44

spherical

Front 45

What is the shape of the p orbital?

Back 45

dumb bell

Front 46

Ion size-Cations

Back 46

-Cations are smaller than their parent atom. Since they have less electrons remaining they are pulled closer to the nucleus. Many times cations lose their outer shell causing a decrease in radius.

Front 47

Ion size-Anions

Back 47

-Anions are larger than their parent atom. Since they have more electrons than protons, electron "pull" is reduced resulting in a larger anion radius in contrast to the neutral atom.

Front 48

isoelectronic

Back 48

Atoms, ions, and molecules containing the same number of electrons.