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Chem 100 > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

chemical symbols

A

one or two letter abbreviations for names of elements

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2
Q

periodic table

A

Arrangement of elements

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3
Q

period

A

horizontal row on the periodic table; there are 7 periods

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4
Q

group

A

vertical column on the periodic table, elements of the same group have similar properties

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5
Q

representative elements

A

Group 1,2 and 13-18 (AKA group numbers 1A-8A)

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6
Q

group numbers

A

1A-8A (from groups 1,2, 13-18)

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7
Q

transition elements

A

center of periodic table (groups 3-12) (group numbers 3B-2B)

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8
Q

alkali metals
conducting of heat and electricity
boiling and melting point?

A

group 1A, with the exception of H

soft, shiny metals, good conductors of heat and electricity, have low boiling and melting points

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9
Q

alkaline earth metals

A

group 2A (2), shiny metals but not as reactive as alkali metals

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10
Q

halogens

A

group 7A- highly reactive

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11
Q

noble gases

A

unreactive

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12
Q 
metals
appearance?
melting point?
solidity?
conduction of heat and electricity?
A

shiny solids, malleable, good conductors of heat and electricity, melt at higher temperatures than nonmetals, solid at room temperature (exception: Mercury is liquid at room tempertature

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13
Q 
Nonmetals
appearance?
density?
solidity?
conduction of heat and electricity?
A

not shiny, ductile or malleable, poor conductors of heat and electricity, low melting points, low density

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14
Q

Metalloids

A

found at zigzag (exception Aluminum); have characteristics of metals and nonmetals, semiconductors

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15
Q

Atom

A

smallest particle of an element

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16
Q

John Dalton’s theory of atoms

A
  1. All matter is made of atoms
  2. All atoms of a given element is similar to one another and different from other elements
  3. Atoms combine to form compounds, all particular compounds contain the same number of atom and same element
  4. chemical reactions involve rearrangement, separation, combination of atoms, atoms can’t be created or destroyed
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17
Q

what produces images of individual atoms?

A

scanning tunneling microscopes (stm)

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18
Q

subatomic particles

A

protons, neutrons, and electrons

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19
Q

Who discovered electrons?

A

JJ Thompson

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20
Q

Electrons

A

negatively charged, determines the physical and chemical properties of an element

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21
Q

protons

A

positively charged particles that are heavier than electrons

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22
Q

What did J.J Thompson and Rutherford discover from the Gold Foil experiment?

A

the nucleus is positively charged

electrons surround the nucleus and travel undisturbed

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23
Q

nucleus

A

positively charged center with protons

24
Q

neutrons

A

neutral particle in the nucleus

25
Q

Atomic mass unit (amu)

A

one twelfth mass of carbon

26
Q

protons, electrons and neutrons in amu

A

protons and neutrons = 1 amu

electrons = 1 amu

27
Q

atomic number

A

equals to the number of protons

28
Q

mass number

A

total number of protons and neutrons

29
Q

isotope

A

same atomic number but different numbers of neutrons

30
Q

atomic mass

A

weighted average of all masses of naturally occurring isotopes of that element

31
Q

How do you calculate atomic mass of an element?

A

mass (amu) * abundance (%/100)= average contribution to element’s mass.

32
Q

energy level

A

occupied by electrons, which has a specific energy,, each energy level has a specific quantum number (n=1-7)

33
Q

which energy level is closer to the nucleus, and which energy level holds more electrons?

A

the lower the energy level: closer to the nucleus.

Higher energy levels hold more electrons.

34
Q

sublevels

A

a group of orbitals within the (principal) energy levels. The number of sub levels is the same as the principal quantum number (n)

35
Q

sublevels from lowest energy level to highest

A

s, p, d, f

36
Q

orbital

A

region around nucleus where electrons of a certain energy are MORE LIKELY to be found

37
Q 
s orbital
shape?
number of orbitals?
as quantum level increases, what happens to the orbitals?
number of total electrons?
A

sphere,
only one s orbital for every energy level starting at n=1,
as principal quantum level increases, s orbitals increase in size.
4 electrons total

38
Q 
p orbital
shape?
number of orbitals?
as quantum level increases, what happens to the orbitals?
number of total electrons?
A

3 orbitals for every sub level starting at n=2
arranges around x,y, and z axes around nucleus(each shaped like a dumbbell)
orbitals increase in volume as n increases
6 electrons total

39
Q

how many electrons can each orbital hold?

A

2 electrons

40
Q

d orbitals
how many orbitals for each sublevel?
max total electrons?

A

5 orbitals

10 electrons

41
Q

f orbitals
how many orbitals?
max total electrons?

A

7 orbitals

14 electrons

42
Q

electron configuration

A

shows placement of electrons in the orbitals in order of increasing energy

43
Q

orbital diagram

A

diagram that shows the distribution of electrons in the orbitals of the energy level

44
Q

s block

A

groups 1A (1) and 2A (2) (includes H and He)

45
Q

p block

A

groups 3A (13)to 8A (18)

46
Q

d block

A

transitional elements, the sub level is (n-1)

47
Q

f black

A

inner transition elements (bottom 2 rows of the periodic table) the sub level is (n-2)

48
Q

Valence electrons

A

determines chemical properties of an element, group # equals number of valence electrons, represented by the highest energy level in s and p orbitals

49
Q

atomic size

A

determined by atomic radius,
atomic size increases as you go down a group
atomic size decreases as you go across a period.
(top right corner= smallest)

50
Q

atomic size periodic table rules exception

A

transitional elements’ atomic radii changes slightly because electrons add to the d orbitals instead of outermost orbitals (s and p)

51
Q

ionization energy

A

energy required to remove a valence electron in the gaseous state

52
Q

ionization energy rules

A

ionization energy decreases as you go down the periodic table
ionization energy increases as you go across the period
(bottom left= smallest)

53
Q

cation

A

when an electron is removed from a neutral atom (due to ionization)

54
Q

what happens when positive charge increases?

A

more ionization energy is required

55
Q

do metals have high ionization energies?

do nonmetals?

A

metals have low ionization and nonmetals have high ionization energies.

56
Q

metallic character

A

elements with high metallic character loses electrons easily

57
Q

metallic character rules on the periodic table

A

metallic character decreases as you go across a period
metallic character increases as you go down a group.
(top right corner= least metallic-ness)

Chem 100 (20 decks)

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