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Chemistry > Ionic Compounds > Flashcards

Ionic Compounds Flashcards

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1
Q

metallic bonding

A

The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons. Electrons move easily from one ion to another. Strongest bond there is

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2
Q

diatomic molecule

A

A molecule containing only two atoms of the same element.

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3
Q

What makes metals good conductors of electricity?

A

They have highly mobile valence electrons.

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4
Q

malleability

A

The ability of a substance to be hammered or beaten into thin sheets.

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5
Q

Ductility

A

The ability of an atom to be drawn, pulled, or extruded through a small opening to produce a wire.

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6
Q

Ionic compound

A

A compound composed of positive and negative ions that are combined so that the number of positive and negative charges are equal.

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7
Q

molecule

A

A neutral group of atoms that are held together by covalent bonds

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8
Q

covalent bond

A

A chemical bond that shares electrons, all diatomic molecules (7,7,7)

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9
Q

one

A

mono

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10
Q

two

A

di

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11
Q

three

A

tri

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12
Q

four

A

tetra

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13
Q

five

A

penta

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14
Q

six

A

hexa

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15
Q

seven

A

hepta

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16
Q

eight

A

octa

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17
Q

nine

A

nona

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18
Q

ten

A

deca

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19
Q

Which of two nonmetals should go first in a covalent compound formula?

A

The least electronegative

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20
Q

which elements form ionic bonds?

A

metal and nonmetal

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21
Q

Which elements form covalent bonds?

A

nonmetal and nonmetal

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22
Q

Which elements form metallic bonds?

A

metal and metal

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23
Q

polar covalent bond

A

When there is an uneven distribution of charges and electrons are attracted by the more electronegative atom

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24
Q

polar covalent bond electronegativity difference

A

0.31-1.7

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25
Q

ionic bond

A

transfer of electrons, electrical attraction between cations and anions

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26
Q

ionic bond electronegativity difference

A

greater than 1.7

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27
Q

non-polar covalent bond electronegativity difference

A

0-0.3

28
Q

chemical bond

A

mutual attraction between the nuclei and valence electrons of different atoms that binds the atoms together

29
Q

ionic compounds are…

A

hard, brittle, good conductors, tend to be soluble in water, has stronger attractions than covalent compounds due to +/- forces, higher boiling/melting points, solids at room temperature

30
Q

covalent compounds are

A

weaker attractions than ionic compounds and have lower boiling/melting points and are gases at room temperature

31
Q

polyatomic ions

A

charged group of covalently bonded atoms

32
Q

boiling point is the same as

A

condensation point

33
Q

boiling according to Paul Hewitt

A

Happens when water molecules are moving fast enough to make a bubble with a higher pressure than the air pressure pushing down on it.

34
Q

boiling typically increases in relation to

A

mass

35
Q

water molecules boil at high temperatures because

A

they are very clingy and have hydrogen bonds

36
Q

hydrogen bond

A

the attraction of the slightly positive side of one molecule to the slightly negative side of ANOTHER molecule.

37
Q

possible hydrogen bond elements

A

nitrogen, oxygen, or fluorine, only happens with polar molecules

38
Q

why are hydrogen bonds not true bonds?

A

There is not sharing or transfer of electrons.

39
Q

Why does water have a spherical shape?

A

It’s a response to the inward forces pulling the molecules together

40
Q

cohesion

A

the attraction of life molecules for each other

41
Q

adhesion

A

the attraction of unlike molecules for one another

42
Q

capillary action

A

when surface tension holds water intact and adhesion causes the water to bond to the walls of a vessel and the entire liquid is dragged upwards, forming a meniscus

43
Q

surface tension

A

the tension of a surface film of a liquid that is under tension

44
Q

is the surface tension in water equal in all directions?

A

No, the molecules at the surface of the water is not completely surrounded by other molecules. This causes them to cohere more strongly to the molecules at the surface so that it acts like a thin elastic membrane.

45
Q

evaporation

A

when individual water molecules gain enough speed to escape the puddle they’re in and go airborne.

46
Q

evaporation leaves behind a hotter or colder puddle?

A

Colder. It takes the higher energy, hotter atoms with it when it leaves

47
Q

condensation leaves behind a hotter or colder puddle?

A

hotter

48
Q

Salt ____ the rate of evaporation

A

decreases

49
Q

Salt ____ the rate of condensation

A

increases

50
Q

what temperature does the volume of water stop decreasing?

A

4 degrees Celsius. The density has reached a maximum and it is as dense as it will ever get. As the temperature is lowered beyond 4 degrees the volume of water begins to expand and the density decreases.

51
Q

When water is cooled, it

A

becomes denser and shrinks

52
Q

solid state is highly

A

organized

53
Q

salt ____ the melting point of water

A

lowers

54
Q

salt ____ the boiling point of water

A

increases

55
Q

exceptions to the octet rule

A

hydrogen, beryllium, and boron

56
Q

boron’s ideal number of valence electrons

A

6

57
Q

hydrogen’s ideal number of valence electrons

A

2

58
Q

beryllium’s ideal number of valence electrons

A

4

59
Q

Which ions require the use of roman numerals?

A

cations in the d block (transition elements) and tin and lead

60
Q

VSPR

A

Valence Shell Electron Pair Repulsion

61
Q

linear shape and example

A

in a line, H2

62
Q

bent

A

bent, water (H2O)

63
Q

trigonal planar

A

boron trihydride

64
Q

trigonal pyramidal

A

ammonia (NH3)

65
Q

tetrahedral

A

methane (CH4)

Chemistry (7 decks)

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