chapter 6 Flashcards
1
Q
- Atoms form ………… charged ions when they lose electrons and ………….. charged ions when
they gain electrons. - ………… bonds occur when the atoms of one element lose valence electrons and the atoms of another element gain valence electrons.
- …………. bonds occur when nonmetal atoms share electrons to attain a noble gas arrangement.
- which type of bond forms between metals and non-metals?
- Which type of bond forms between non-metals?
A
- positively, negatively
- ionic
- covalent
- ionic
- covalent
2
Q
- ions of elements in groups 1A, 2A, and 3A have what kind of charge? Why?
- What are the charges of groups 1A to 3A? Why?
- What are the charges of groups 5A to 7A? Why?
- How do we name ions?
- Are cations smaller or larger than atoms of the same element? Why? Anions?
- Cations lose electrons until ……….. What about anions?
A
- positive because they are losing electrons, thus having a greater number of protons to electrons.
- 1A=1+, 2A=2+, 3A=3+ because ionization energy is low and they give their electrons away easily.
- 5A=3-, 6A=2-, 7A=1- because ionization energy is high and they pull electrons away from other atoms.
- The cation retains the element name. The anion will now end in “ide” example: NaCl sodium chloride
- cations are smaller because they lost electrons. Anions are larger because they gained electrons.
- they have the same number of valence electrons as the nearest noble gas, usually eight valence electrons. Anions do exactly the opposite (gain electrons).
3
Q
- What are 3 characteristics of ionic bonds?
- What is another name for ionic bonds?
- What is denoted in the superscript? The subscript?
A
- they have high melting points, are cystalline, rigid, and are aqueous (can conduct). As solids, they are good insulators
- electrovalent
- The charge of the ion. The number of ions.
4
Q
- Transition metals except for (which 3 elements) form two or more positive ions (cations). What are the charges for these 3 elements?
A
- Zinc, cadmium, and silver. Charges: Zn2+, Cd2+, and Ag+
5
Q
Name the 11 transitional metals with variable charges, and what those charges are:
A
- Bismuth: Bi3+, and Bi5+
- Chromium Cr2+, and Cr3+
- Cobalt Co2+, and Co3+
- Copper Cu+, and Cu2+
- Gold Au+, and Au3+
- Iron Fe2+, and Fe3+
- Lead Pb2+, and Pb4+
- Manganese Mn2+, and Mn3+
- Mercury Hg2+
- Nickle Ni2+, and Ni3+
- Tin Sn2+, and Sn4+
6
Q
- All transitional metals have a ………….. charge.
2. How do we name transitional metal ions?
A
- positive
2. We put the charge in roman numerals in parentheses after the element name: Bismuth (III).
7
Q
- What are polyatomic ions?
2. What are their charges usually? Which polyatomic ion is the exception to this?
A
- a group of atoms with an overall charge
often consisting of a nonmetal—such as phosphorus, sulfur, carbon, or nitrogen—and oxygen - Negative charges of 1-, 2-, 3-. The exception is NH4+ ammonium
8
Q
Give the names and formulas for the following polyatomic ions:
- Hydrogen
- Nitrogen
- Chlorine
- Carbon
- Sulphur
- Phosphorus
- Iodine and bromine?
- If a polyatomic ion has one less Oxygen than the “ate”, what does it become? If it has two less? What if it contains an H?
A
- OH- Hydroxide
- NH4+ Ammonium, NO3- Nitrate
- ClO4- Perchlorate, ClO3- Chlorate
- CO3^2- carbonate, CN- cyanide, C2H3O2- Acetate
- SO4^2- Sulfate
- PO4^3- phosphate
- same as chlorine
- it becomes an “ite”, two less becomes a “hypo-ite”. The H signifies hydrogen.
9
Q
- How do you signify that more than one polyatomic ion is needed to balance a charge?
- When an H is added to a polyatomic ion, what happens?
A
- Put parentheses around the polyatomic ion and outside of the parentheses, put the subscript: Mg(NO3)2
- The polyatomic ion gets a 1+ positive charge. For example: SO4^2 becomes HSO4-
10
Q
- What is a molecular compound?
- The number of covalent bonds that a nonmetal atom forms is usually ……………….
- How do we name molecular compounds?
- What are the prefixes for more than one atom of an element in a molecular compound?
A
- a compound that contains 2 or more non-metals that form covalent bonds.
- equal to the number of electrons it needs to achieve a stable electron arrangement
- the first nonmetal in the formula is named by its element name, the second nonmetal is named by using the first syllable of its name followed by ide. If a subscript is used in the formula, a prefix is used in front of its name
- mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
11
Q
- What is a diatomic molecule?
2. Name the 7 diatomic molecules
A
- an element that only exists in a duo. For example O2. You never find just O.
- hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine.
12
Q
A compound is usually ………… if the first element in the formula is a metal or the polyatomic ion NH4+ . It is …………… if the first element in the formula is a nonmetal.
A
ionic, covalent
13
Q
- Electronegativity ……………. from left to right going across a period. Electronegativity …………. from the bottom to the top of the periodic table. Electronegativity is …….. for the nonmetals, with ……… as the highest. Electronegativity is …. for the metals.
- rate the different types of bonds in order of increasing electronegativity.
- What are the numerical ranges for amounts of electronegativity?
A
- increases, increases, high, fluorine, low
- non-polar covalent, polar covalent, ionic
- 0-0.4 is non-polar. 0.5-1.8 is polar, >1.8 is ionic
14
Q
- What are the 4 kinds of attractive forces between particles, and list in order of increasing strength of attraction?
- Are melting points higher or lower for different bonds?
A
- Dispersion Forces: temporary dipoles as electrons move around causing temporary differences in electronegativity. They make solid and liquid states possible. (non-polar covalent).
- Dipole-dipole (positive end of one molecule and negative end of the other). Dogs sniffing each other’s butts (polar covalent)
- Hydrogen bonds. These happen between Hydrogen bonding with either fluorine, oxygen, or nitrogen. The sluttiness of hydrogen makes it easy to bond with everything around. Strongest type of polar covalent bond.
- Ionic bonds. Have highest melting points. Strongest type of bonds.
- The stronger the bond, the higher the melting point.
15
Q
- The positive and negative ends of the dipole are located by using ……… or ………….. .
A
- the lowercase Greek letter delta with a positive or negative charge or an arrow that points from the positive to the negative end of the dipole (vector).
