Chapter 3

Question 1

chemical symbols

Answer 1

one or two letter abbreviations for names of elements

Question 2

periodic table

Answer 2

Arrangement of elements

Question 3

period

Answer 3

horizontal row on the periodic table; there are 7 periods

Question 4

group

Answer 4

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

Question 5

representative elements

Answer 5

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

Question 6

group numbers

Answer 6

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

Question 7

transition elements

Answer 7

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

Question 8

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

Answer 8

group 1A, with the exception of H

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

Question 9

alkaline earth metals

Answer 9

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

Question 10

halogens

Answer 10

group 7A- highly reactive

Question 11

noble gases

Answer 11

unreactive

Question 12

metals
appearance?
melting point?
solidity?
conduction of heat and electricity?

Answer 12

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

Question 13

Nonmetals
appearance?
density?
solidity?
conduction of heat and electricity?

Answer 13

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

Question 14

Metalloids

Answer 14

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

Question 15

Atom

Answer 15

smallest particle of an element

Question 16

John Dalton’s theory of atoms

Answer 16

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

Question 17

what produces images of individual atoms?

Answer 17

scanning tunneling microscopes (stm)

Question 18

subatomic particles

Answer 18

protons, neutrons, and electrons

Question 19

Who discovered electrons?

Answer 19

JJ Thompson

Question 20

Electrons

Answer 20

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

Question 21

protons

Answer 21

positively charged particles that are heavier than electrons

Question 22

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

Answer 22

the nucleus is positively charged

electrons surround the nucleus and travel undisturbed

Question 23

nucleus

Answer 23

positively charged center with protons

Question 24

neutrons

Answer 24

neutral particle in the nucleus

Question 25

Atomic mass unit (amu)

Answer 25

one twelfth mass of carbon

Question 26

protons, electrons and neutrons in amu

Answer 26

protons and neutrons = 1 amu | electrons = 1 amu

Question 27

atomic number

Answer 27

equals to the number of protons

Question 28

mass number

Answer 28

total number of protons and neutrons

Question 29

isotope

Answer 29

same atomic number but different numbers of neutrons

Question 30

atomic mass

Answer 30

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

Question 31

How do you calculate atomic mass of an element?

Answer 31

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

Question 32

energy level

Answer 32

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

Question 33

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

Answer 33

the lower the energy level: closer to the nucleus. | Higher energy levels hold more electrons.

Question 34

sublevels

Answer 34

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

Question 35

sublevels from lowest energy level to highest

Answer 35

s, p, d, f

Question 36

orbital

Answer 36

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

Question 37

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

Answer 37

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

Question 38

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

Answer 38

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

Question 39

how many electrons can each orbital hold?

Answer 39

2 electrons

Question 40

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

Answer 40

5 orbitals | 10 electrons

Question 41

f orbitals how many orbitals? max total electrons?

Answer 41

7 orbitals | 14 electrons

Question 42

electron configuration

Answer 42

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

Question 43

orbital diagram

Answer 43

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

Question 44

s block

Answer 44

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

Question 45

p block

Answer 45

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

Question 46

d block

Answer 46

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

Question 47

f black

Answer 47

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

Question 48

Valence electrons

Answer 48

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

Question 49

atomic size

Answer 49

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)

Question 50

atomic size periodic table rules exception

Answer 50

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

Question 51

ionization energy

Answer 51

energy required to remove a valence electron in the gaseous state

Question 52

ionization energy rules

Answer 52

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

Question 53

cation

Answer 53

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

Question 54

what happens when positive charge increases?

Answer 54

more ionization energy is required

Question 55

do metals have high ionization energies? | do nonmetals?

Answer 55

metals have low ionization and nonmetals have high ionization energies.

Question 56

metallic character

Answer 56

elements with high metallic character loses electrons easily

Question 57

metallic character rules on the periodic table

Answer 57

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