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Chemistry 1 > Unit 3 Periodic Table > Flashcards

Unit 3 Periodic Table Flashcards

1
Q

Left side of the periodic table:

A

metals

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2
Q

malleable, ductile

A

metals

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3
Q

good conductors of electricity

A

metals

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4
Q

most are solid at room temperature (except for mercury)

A

metals

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5
Q

right side of periodic table (and hydrogen)

A

nonmetals

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6
Q

brittle

A

nonmetals

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7
Q

most are gas at room temperature

A

nonmetals

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8
Q

located along stair step of periodic table

A

metalloids

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9
Q

semiconductors

A

metalloids

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10
Q

Periods

A

horizontal rows on the periodic table

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11
Q

Groups

A

vertical columns on the periodic table (also called families)

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12
Q

what groups are transition metals

A

groups 3-12 or B groups

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13
Q

transition metals are _____ luster

A

high

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14
Q

inner transition metals

A

lanthanides: bellow periodic table (first row)
actinides: bellow periodic table (second row)

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15
Q

Halogens

A

Group 17
-most reactive nonmetals

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16
Q

Nobel Gases

A

group 18
-Stable atoms that don’t bond with other elements (inert)
-nonflammable and nonreactive

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17
Q

Alkali metals

A

first group of periodic tables
-most reactive metals

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18
Q

where are Alkaline Earth metals

A

group 2 in periodic table

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19
Q

Electron Cloud

A

area round nucleus where electrons are likely to be found.

20
Q

Orbitals

A

3d regions around the nucleus that describe probable locations of electrons

21
Q

What are the four types of sublevels?

A

s, p, d, f

22
Q

how many orbitals dose each sublevel have?

A

s=1
p=3
d=5
f=7

23
Q

How many electrons can each sublevel hold?

A

s=2
p=6
d=10
f=14

24
Q

each orbital can hold ___ electrons?

A

2

25
Q

Electron Configuration

A

the arrangement of electrons in an atom

26
Q

An electron occupies the ________ energy orbital that can receive it.

A

lowest

27
Q

2 electrons that occupy the same orbital must have ______ ___________.

A

opposite spins

28
Q

How do orbitals of the same energy fill up?

A

each orbital is occupied by 1 electron before any orbital is occupied by a 2nd electron.

29
Q

In the Sublevel 3s^2 what dose “3” represent

A

3 represents the energy level.

30
Q

Valence Electrons

A

the electrons in the outermost energy level (energy shell)

31
Q

Oxidation number

A

the charge of an ion

32
Q

stable

A

an atom with a full outer energy shell

33
Q

period number =

A

the number of energy levels

34
Q

for non-transition elements, group number=

A

number of valence electrons

35
Q

For transition metals, the number of valence electrons is:

A

all electrons in the highest value of n (energy level), and unfilled d or f shells

36
Q

Octet rule-

A

chemical compounds form so that each atom has a full set of electrons in its highest energy level.

37
Q

Trend in atomic radius and atomic character across the periodic table:

A

increases as you go down the periodic table
decreases as you go from left to right

38
Q

Trend in electronegativity and ionization energy across the periodic table:

A

decreases as you go down the periodic table
increases as you go from left to right

39
Q

Cation

A

a positive ion
-metals from cations

40
Q

Anion

A

a negative ion
-nonmetals from anions

41
Q

Ionization energy (IE)

A

energy needed to remove an electron from a neutral ion
-the greater the number the harder it is to remove an electron

42
Q

Each successive electron removed requires ________ energy.

A

more

43
Q

electronegativity

A

the ability of an atom to attract electrons.

44
Q

metalic character

A

ser of chemical properties associated with metal on the periodic table.
-ability to lose electrons (easily achieve octet)
-low ionization energy
-low electronegativity

45
Q

Most metallic elements

A

bottom left

46
Q

What elements along the stair of the periodic table are not Metalloids?

A

Aluminum (Al), Astatine (At)

Chemistry 1 (6 decks)

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