chap 6 Flashcards

1
Q

going down a group of the periodic table what patterns would you notice?

A
  • atomic size increases
  • ionic size increases
  • ionization enegry decreases
  • electronegativity decreases
  • nuclear charge increases
  • shielding increases
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2
Q

Going across a period what patterns would you notice?

A
  • Atomic size decreases
  • ionization energy increases
  • electronegativity increases
  • nuclear charge increases
  • shielding is constant
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3
Q

elements were first classified according to what

A

their properties

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4
Q

who created the periodic table

A

Mendeleev

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5
Q

on mendeleevs periodic table how were elements placed

A

in increasing atomic mass

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6
Q

what did Mendeleev discover thru his table

A

the properties of unknown elenments

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7
Q

what is the modern day table organized by

A

atomic number

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8
Q

metals are…

A

good conductors and many are ductile and malleable

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9
Q

nonmetals are…

A

mostly gase whose properties are opposite to those of metals

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10
Q

metaloids can…

A

behave like metals or nonmetals depending on condition

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11
Q

How many elements had been identified by the year 1700?

A

13

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12
Q

What caused the rate of discovery to increase after 1700?

A

Chemists began to use scientific methods to search for elements

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13
Q

What did chemists use to sort elements into groups?

A

Chemists used the properties of elements.

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14
Q

Who was Dmitri Mendeleev?

A

he created a periodic table

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15
Q

What property did Mendeleev use to organize the elements into a periodic table?

A

arranged the elements in order of increasing atomic mas

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16
Q

what are 3 things u can name by looking at an element on the periodic table

A
  • atomic number
  • atomic mass
  • what type of element it is
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17
Q

what is a valence electron

A

outer edge

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18
Q

Why are Group A elements called representative elements?

A

They exhibit a wide range of physical and chemical properties

19
Q

Description of Electron Configuration for noble gases

A

s or p sublevels are filled

20
Q

Description of Electron Configuration for Representative elements

A

s or p sublevels are only partially filled

21
Q

Description of Electron Configuration for transition metals

A

s sublevel and nearby d sublevel contain electrons

22
Q

Description of Electron Configuration for inner transition metals

A

s sublevel and nearby f sublevel contain electrons

23
Q

letter of the elements found in the p block

A

Groups 3A, 4A, 5A, 6A, 7A, and 8A except helium

24
Q

Ions form when…

A

atoms gain or lose electrons.

25
Q

A positively charged cation forms

A

when an atom loses one or more electrons.

26
Q

negatively charged anion forms

A

s when an atom gains one or more electrons.

27
Q

First ionization energy

A

is the amount of energy required to remove one electron from
a neutral atom

28
Q

Ionization energy tends to decrease from

A

top to bottom within a group
an
increase from left to right across a period.

29
Q

A cation is

A

smaller than the atom that formed it

30
Q

an anion

A

is larger than the atom that
formed it.

31
Q

Ionic size generally increases

A

from top to bottom within a group

32
Q

Ionic size generally decreases

A

from left to right across a period.

33
Q

Electronegativity tends to decrease from

A

top to bottom

34
Q

Electronegativity tends to increase from

A

from left to right across a period.

35
Q

What is the general trend in atomic size within a group?

A

The atomic size increases within a group as atomic number increases. The atomic size
decreases from left to right across a period

36
Q

What are the two variables that affect atomic size within a group?

A
  • the charge on the nucleus
  • the number of occupied energy levels
37
Q

What is an ion?

A

an atom or group of atoms that has a positive or negative charge

38
Q

How are ions formed

A

An ion is formed when electrons are transferred between atoms.

39
Q

An ion with a positive charge is called a(n)

A

cation

40
Q

an ion with a negative
charge is called a(n)

A

anion

41
Q

anions

A
  • neg
  • nonmetal
  • minus sign
42
Q

cations

A
  • pos
  • metal
  • plus sign
43
Q

Why does ionization energy tend to decrease from top to bottom within a group?

A

Atomic size increases from top to bottom within a group. The nuclear charge
has a smaller effect on the electrons in the highest occupied energy level, so less
energy is required to remove an electron.